organizing the periodic table - mrs. gross's...
TRANSCRIPT
![Page 1: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/1.jpg)
![Page 2: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/2.jpg)
Organizing the Periodic Table
How did chemists begin to organize the
known elements?
Chemists used the properties of the
elements to sort them into groups.
![Page 3: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/3.jpg)
The Organizers
JW Dobereiner
grouped the elements into triads.
Problem: Not all of the elements could
be put into triads.
![Page 4: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/4.jpg)
The Organizers
Dmitri Mendeleev
arranged the elements by
increasing atomic mass.
Problem: the chemical properties of
the elements did not line up correctly.
![Page 5: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/5.jpg)
Pg. 156
Figure
6.3
![Page 6: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/6.jpg)
The Organizers
Lother Meyer
also created a periodic table similar to
Mendeleev’s, however Mendeleev
published his table first and could
explain his table better.
![Page 7: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/7.jpg)
Development of Atomic Theory
The structure of the atom was
determined through years of
experimentation. Once the structure
of the atom was determined by Dalton,
Thomson, Rutherford, Chadwick, Bohr,
and others, Henry Moseley
determined the atomic number for
the elements.
![Page 8: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/8.jpg)
Organization of
Modern Periodic Table
The elements are arranged
in order of
increasing atomic number.
![Page 9: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/9.jpg)
Periodic Law
When elements are arranged in
order of increasing atomic
number, there is a periodic
repetition of their physical and
chemical properties.
![Page 10: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/10.jpg)
Three classes of elements:
Metals
Nonmetals
Metalloids
Across a period, the properties of
elements become less metallic and
more nonmetallic.
![Page 11: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/11.jpg)
![Page 12: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/12.jpg)
Properties of Metals
•Solids (except for Hg) at room temperature
•Make up 80% of the periodic table
•Good conductors of heat and electricity
•Shiny
•Ductile (can be made into thin wire)
•Malleable (can be hammered into sheets)
![Page 13: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/13.jpg)
Properties of Nonmetals
Properties vary among the nonmetals.
At room temperature, some are gases,
some are solids, and 1 is a liquid.
•Poor conductors
•Brittle
•Not ductile
•Not malleable
![Page 14: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/14.jpg)
Metalloids (Semi-metals)
B, Si, Ge, As, Sb, Te, At
Behave like metals under certain
conditions.
Behave like nonmetals under
different conditions.
![Page 15: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/15.jpg)
Which of these sets of elements have
similar physical and chemical properties?
a. oxygen, nitrogen, carbon, boron
b. strontium, magnesium, calcium, beryllium
c. nitrogen, neon, nickel, niobium
![Page 16: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/16.jpg)
Identify each element as a metal,
metalloid, or nonmetal.
a. gold
b. silicon
c. sulfur
d. barium
![Page 17: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/17.jpg)
Name two elements that have
properties similar to those of the
element sodium.
![Page 18: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/18.jpg)
What pattern is revealed when the
elements are arranged in a periodic table
in order of increasing atomic number?
![Page 19: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/19.jpg)
Identify each property below as more
characteristic of a metal or a nonmetal.
a. a gas at room temperature
b. brittle
c. malleable
d. poor conductor of electric current
e. shiny
![Page 20: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/20.jpg)
In general, how are metalloids different
from metals and nonmetals?
![Page 21: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/21.jpg)
Representative Elements
Elements in columns
1, 2, 13, 14, 15, 16, 17, 18
OR
Elements in columns
1A, 2A, 3A, 4A, 5A, 6A, 7A, 8A
OR
Elements in blocks s and p
![Page 22: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/22.jpg)
Representative Elements
Called “REPRESENTATIVE”
elements because they display a
wide range of chemical and
physical properties.
![Page 23: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/23.jpg)
Which of the following are symbols for
representative elements:
Na, Mg, Fe, Ni, Cl ?
![Page 24: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/24.jpg)
Transition Metals
Elements in columns
3, 4, 5, 6, 7, 8, 9, 10, 11, 12
OR
Elements in columns
3B, 4B, 5B, 6B, 7B, 8B, 1B, 2B
OR
Elements in the d block
![Page 25: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/25.jpg)
Transition Metals
Characterized by electrons
filling the d orbitals
When transition metal ions form compounds,
the compounds often exhibit various colors.
Iron oxide Red
Cadmium sulfate Orange
Copper(II) chloride Blue-green
![Page 26: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/26.jpg)
Inner Transition Metals (Rare earth elements)
Elements in the f block
Consists of the
Lanthanide (La) series
and the
Actinide (Ac) series.
![Page 27: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/27.jpg)
Inner Transition Metals (Rare earth elements)
Contains some elements that occur
naturally
and some that are synthetic.
Some are radioactive, some are not.
![Page 28: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/28.jpg)
Groups in the Periodic Table
Alkali metals – column 1 (or 1A)
Alkaline earth metals – column 2 (or 2A)
Halogens (salt-formers) – column 17 (7A)
Noble gases – column 18 (or 8A)
![Page 29: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/29.jpg)
Why do the elements potassium and
sodium have similar chemical properties?
![Page 30: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/30.jpg)
Classify each element as a
representative element, transition
metal, or noble gas.
a. 1s22s22p63s23p64s23d104p6
b. 1s22s22p63s23p64s23d6
c. 1s22s22p63s23p2
![Page 31: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/31.jpg)
Which of the following elements are
transition metals:
Cu, Sr, Cd, Au, Al, Ge, Co ?
![Page 32: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/32.jpg)
How many electrons are in the
highest occupied energy level of a
Group 5A element?
![Page 33: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/33.jpg)
Trends
in the
Periodic
Table
![Page 34: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/34.jpg)
Shielding is the result of the core
electrons blocking the ‘pull’ of the
nucleus on the outermost electrons.
Terms to Know
Nuclear charge is the charge
in the nucleus.
![Page 35: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/35.jpg)
Terms to Know
Atomic Radius is one half the distance
between the nuclei of two atoms of the
same element when the atoms are joined.
Pg. 170 Figure 6.13
![Page 36: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/36.jpg)
Atomic Radius
From left to right across a period,
the atomic radius generally decreases.
Why? As you go across a row, there is an increase
in the number of protons and the number of electrons.
However, the electrons being added are added to the
same principle energy level, so the shielding remains
the same. Therefore, the increased nuclear charge
pulls the outermost electrons in closer to the nucleus.
The result is a smaller atom.
(See pg. 171, 3rd paragraph.)
![Page 37: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/37.jpg)
Atomic Radius
From top to bottom down a group, the
atomic radius generally increases.
Why? As you go down a column, there is an
increase in the number of protons and the number of
occupied energy levels. The increase in positive
charge pulls the electrons closer to the nucleus, but
the increase in the number of occupied orbitals
shields the nucleus more. The shielding effect is
greater than the increased nuclear charge. The
result is a larger atom.
(See pg. 171, 1st and 2nd paragraph.)
![Page 38: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/38.jpg)
Which element in each pair has atoms
with a larger atomic radius?
a. sodium, lithium
b. strontium, magnesium
c. carbon, germanium
d. selenium, oxygen
![Page 39: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/39.jpg)
Explain why fluorine has a smaller atomic
radius than both oxygen and chlorine.
![Page 40: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/40.jpg)
Terms to Know
Ion is a neutral atom that has either lost
or gained an electron.
Atoms that have gained electrons are
called
Atoms that have lost electron(s) are called
Positive Ions or Cations
Negative Ions or Anions
![Page 41: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/41.jpg)
Cation is an ion that has lost one or
more electrons resulting in a net
positive charge.
![Page 42: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/42.jpg)
Anion is an ion that has gained one
or more electrons resulting in a net
negative charge.
![Page 43: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/43.jpg)
Ion Size
Cations are always
SMALLER than the atoms
from which they form.
Why? When a metal atom loses an electron,
the attraction between the remaining electrons
and the nucleus is increased. The electrons are
drawn closer to the nucleus.
(See pg. 176, 2nd paragraph)
![Page 44: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/44.jpg)
Ion Size
Anions are always
LARGER than the atoms
from which they form.
Why? As the number of electrons
increases, the attraction of the nucleus
for any one electron decreases.
(See pg. 176, 3rd paragraph)
![Page 45: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/45.jpg)
Li F O N C B Be
Li1+ F1- O2- N3- C B3+ Be2+
![Page 46: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/46.jpg)
Ion Trends
From left to right across a period, the
cation size decreases.
From left to right across a period, the
anion size decreases.
(See figure 6.20 on pg. 176)
![Page 47: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/47.jpg)
Pg. 176 Figure 6.20
![Page 48: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/48.jpg)
From top to bottom down a group,
the ionic size increases.
(Pg. 172)
Ion Trends
![Page 49: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/49.jpg)
Which particle has the larger
radius in each atom/ion pair?
a. Na, Na+
b. S, S2-
c. I, I-
d. Al, Al3+
![Page 50: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/50.jpg)
In each pair, which ion is larger?
a. Ca2+, Mg2+
b. Cl - , P3-
c. Cu+, Cu2+
![Page 51: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/51.jpg)
The atomic radius _____________ from
left to right across the periodic table.
The atomic radius ____________
from top to bottom on the period table.
Aside from the noble gases, what is the
smallest atom on the periodic table?
Aside from the noble gases, what is the
largest atom on the periodic table?
![Page 52: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/52.jpg)
The atom is _________ than its cation.
The atom is _________ than its anion.
Cations are _________ than the
anions that are in the same row.
The cation trend from left to right is
that the ionic radius ____________.
The anion trend from left to right is
that the ionic radius _____________.
![Page 53: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/53.jpg)
List the following from smallest to
largest according atomic radius.
a. Mg, S, Na, Si
b. Be, Ba, Ca, Ra
c. F, As, Br, Ga, Cl
List the following from smallest to
largest according ionic radius.
a. Mg2+, S2-, Na+, Cl-
b. Be2+, Ba2+, Ca2+, Ra2+
c. F-, As3-, Br-, Ga3+, Cl-
![Page 54: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/54.jpg)
Terms to Know
Ionization
Energy
is the energy
required to
remove an
electron
from an
atom. (Pg. 173-175)
![Page 55: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/55.jpg)
Explain the difference between the terms
“first ionization energy” and “second
ionization energy” of an element.
The first ionization energy is the energy
needed to remove a first electron from an
atom.
The second ionization energy is the energy
needed to remove a second electron.
![Page 56: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/56.jpg)
Why is there a large increase between the
first and second ionization energies of the
alkali metals?
It is relatively easy to remove the first
electron from an alkali metal atom because
they have only one valence electron;
it is much more difficult to remove the
second because it is being removed from a
full energy level.
![Page 57: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/57.jpg)
There is a large jump between the
second and third ionization energies
of magnesium. There is a large jump
between the third and fourth
ionization energies of aluminum.
Explain these observations.
![Page 58: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/58.jpg)
It is relatively easy to remove two electrons
from magnesium because it has 2 valence
electrons; it is much more difficult to remove a
third electron because it comes from a full
energy level.
It is relatively easy to remove three electrons
from aluminum because it has 3 valence
electrons; it is much more difficult to remove a
fourth electron because it comes from a full
energy level.
![Page 59: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/59.jpg)
Ionization Energy
From left to right across a period,
the ionization energy generally
increases.
Why? As you go across a row, there is an increase
in the nuclear charge, but the shielding effect remains
the same. There is an increase in the attraction of the
nucleus for an electron. Thus it takes more energy to
remove an electron from the atom.
(See pg. 174, 2nd paragraph.)
![Page 60: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/60.jpg)
From top to bottom down a group,
the ionization energy generally
decreases.
Why? As the size of the atom increases and the
amount of shielding electrons increases, nuclear
charge has a smaller effect on the electrons in the
outermost energy level. Therefore, less energy is
required to remove an electron from the outermost
energy level.
(See pg. 174, 1st paragraph.)
Ionization Energy
![Page 61: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/61.jpg)
Which element in each pair has a
greater first ionization energy?
a. lithium, boron
b. magnesium, strontium
c. cesium, aluminum
![Page 62: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/62.jpg)
Would you expect metals or nonmetals in
the same period to have higher ionization
energies? Give a reason for your answer.
![Page 63: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/63.jpg)
Explain each of the following comparisons.
Calcium has a smaller second ionization
energy than does potassium.
![Page 64: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/64.jpg)
Explain each of the following comparison.
Lithium has a larger first ionization
energy than does cesium.
![Page 65: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/65.jpg)
Explain the following comparison.
Magnesium has a larger third
ionization energy than does aluminum.
![Page 66: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/66.jpg)
Electronegativity
Electronegativity
is the ability of an atom to attract
electrons when the atom is in a
compound.
(See pg. 177, 1st paragraph)
![Page 67: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/67.jpg)
For the representative elements:
From top to bottom down a group,
the electronegativity values decrease.
(See pg. 177, 3rd paragraph)
From left to right across a period,
the electronegativity values increase.
Electronegativity
![Page 68: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/68.jpg)
Electronegativity
Fluorine is the most electronegative
element on the periodic table.
Why are the noble gases NOT included
in electronegativity table?
Because they are UNREACTIVE and
do NOT want to bond with any atoms.
![Page 69: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/69.jpg)
![Page 70: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/70.jpg)
Which element in each pair has a
higher electronegativity value?
a. Cl, F
b. C, N
c. Mg, Ne
d. As, Ca
![Page 71: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/71.jpg)
When the elements in each pair
are chemically combined, which
element in each pair has a
greater attraction for electrons?
a. Ca or O
b. O or F
c. H or O
d. K or S
![Page 72: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/72.jpg)
Pg. 171
Figure 6.14
![Page 73: Organizing the Periodic Table - Mrs. Gross's Webpage205gross.weebly.com/uploads/2/3/1/4/23146132/chapter_6-1_thru_6-4.pdf · Organizing the Periodic Table How did chemists begin to](https://reader031.vdocuments.us/reader031/viewer/2022042006/5e7019356035b52a1e7c0cc2/html5/thumbnails/73.jpg)
Pg. 174
Figure 6.17