a guided tour of the periodic table section 3.2. using the periodic table atomic number – the...
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A Guided Tour of the Periodic Table
Section 3.2
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Using the Periodic Table
Atomic number – the number of protons in the nucleus of an atom or the number of electrons in the nucleus of an atom.
ALWAYS TRUE!!!!!
The elements are in
order of Periodic Table
by the # of protons present
in the nucleus.
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Using the Periodic Table
Mass number – the TOTAL number of protons and neutrons in the nucleus of an atom; may change.
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Using the Periodic Table
Ions: 1. Ionization – the process of adding electrons
to or removing electrons from an atom or group of atoms.
2. Ion – an atom or group of atoms that has lost or gained one or more electrons and therefore has a net electric charge.
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Using the Periodic Table
Ions:Cation – an ion with a positive charge. (Lithium, Li)
Li+
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IonsAnion – an ion with a negative charge (Flourine, F)
F-
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Using the Periodic Table
Isotopes- any atoms having the same number of protons but DIFFERENT number of neutrons.
See fig 3-17 on pg 84 in textbook
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SymbolAtomic Mass
Atomic Number
Charge (if ion)
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HHydrogen
1
1
Protons: 1Neutrons: 0Electrons: 1
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NaSodium
23
11
Protons: 11Neutrons: 12Electrons: 11
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EXAMPLEHow many protons, neutrons and electrons are found in an atom of
13355 Cs
Atomic number = protons and electronsThere are 55 protons and 55 electrons
Mass number = sum of protons and neutrons133 – 55 = 78
There are 78 neutrons
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Atomic Mass Unit (AMU) – a quantity equal to 1/12 of the mass of a Carbon-12 atom
Average Atomic Mass- the weighted average of the masses of all naturally occurring isotopes of an element.
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Organization of the P.T.
Periodic Law: properties of elements tend to change in a regular pattern when elements are arranged in order of increasing atomic number, or number of protons in their atoms.
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The Periodic Table
Over 100 years ago, the
chemist Mendeleev arranged
the known elements in order
of increasing atomic mass.
He noticed a repeating pattern in the
properties of the elements.
He designed a table with rows and columns to
show the repeating patterns.
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Mendeleev left blank spaces in his table when the properties of the elements above and below did not seem to match.
The existence of unknown elements was predicted by Mendeleev on the basis of the blank spaces.
When the unknown elements were discovered, it was found that Mendeleev had closely predicted the properties of the elements as well as their discovery.
The Periodic Table
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In the Modern Periodic Table . . .
Elements are arranged by increasing atomic numbers.
The term “periodic” part means that similar properties repeat every so often.
There are currently 118 known elements.
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Rows of the Periodic Table
The beginning of the row is where the patterns that Mendeleev discovered begin repeating again.
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What the table tells you . . .
Each box contains information about one of the elements.
- Atomic Number- Chemical Symbol- Name of Element- Atomic Mass
Some tables give more information for each element.
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Periodic Table
The color of the box tells you if the state of the element at room temperature and pressure is a solid, liquid, or gas.
Most are solids, some are gases, and two are liquids.
The stair-step line separates metals from non-metals.
Metals are to the left of the stair-step line; non-metals are to the right.
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Using the Periodic Table
1. Period a horizontal row of elements in the periodic table
2. Determines electron arrangement
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Using the Periodic Table
Groups (family) – a vertical column of elements in the periodic table.
Same number of valence electrons in each group therefore they have similar properties.
Examples: Cl (Chlorine) and F (Flourine)
These are both Halogens and have very similar properties.
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Columns on the Periodic Table
There are 18
columns or
groups.
The elements in
each group
resemble each
other – the react
similarly to other
substances.
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How are elements classified?
A: Metals vs. Nonmetals
1: Elements can be put in various types of categories based on their physical and chemical properties.
A common physical property used to classify elements are metallic and nonmetallic properties.
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Periodic Table: Metallic arrangement
Layout of the Periodic Table: Metals vs. nonmetals1
IA18
VIIIA
12
IIA13
IIIA14
IVA15VA
16VIA
17VIIA
2
33
IIIB4
IVB5
VB6
VIB7
VIIB8 9
VIIIB10 11
IB12IIB
4
5
6
7
MetalsNonmetals
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Periodic Table: The three broad ClassesMain, Transition, Rare Earth
Main (Representative), Transition metals, lanthanides and actinides (rare earth)
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Metals vs Nonmetals
Metallic properties include:
A. Shiny
B. Conduct Heat/Electricity
C. Ductile/Malleable
D. Have a positive Oxidation Number
E. Found on the Left/Middle of the Periodic Table
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Metals vs Nonmetals
Nonmetallic properties include:
a. Dull
b. Poor conductor of Heat/Electricity (INSULATORS)
c. Brittle
d. Have a Negative Oxidation Number
e. Found on the Right Side of P.T.
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Metals vs Nonmetals
Some elements have properties of both metals and nonmetals and are referred to as metalloids.
Metalloids are usually nonmetals that can conduct heat and electricity.
The metalloids are located between the metal and nonmetal sides of the periodic table.
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Metals vs Nonmetals
There are 109 total elements on the periodic table.
Out of the 109 elements, 84 are metals, 17 nonmetals and 8 metalloids (semiconductors)
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Families
FAMILIES OF ELEMENTS
Elements are put into families based on similarities of chemical properties.
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Families
Families of Periodic Table
a. ALKALI METALS – 1 (IA)
b. ALKALINE EARTH METALS – 2 (IIA)
c. TRANSITION METALS – 3-12 (B Groups)
d. HALOGEN GROUP – 17 (VIIA)
e. NOBLE GASES – 18 (VIIIA)
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ALKALIE METALS (IA)
Group IA elements on P.T. With EXCEPTION of Hydrogen (H), they are the
MOST Metallic elements on the table. Best conductors of heat and electricity Most reactive metals on earth Never found free, always found in a
compound.
ALL HAVE ONLY 1 VALENCE ELECTRON
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Alkaline Earth Metals (IIA)
Group IIA on P.T. Not as reactive as the group IA metals Still very reactive Never found free in natureALL HAVE 2 VALENCE ELECTRONS
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TRANSITION METALS (IIIB – IIB)
A majority of the elements on the periodic table are transition metals.
Names given based on their decreasing metallic characteristics as one moves from the left to the right side of the periodic table.
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HALOGENS
Found in group VIIA Known as the Salt Forming elements HALO- means “salt forming” Most reactive nonmetals NEVER found free in nature Usually found in salt compounds containing
a metal from either alkali or alkaline earth metal families.
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NOBLE GASES
Group VIIIA ALL Nonreactive Nonmetals Only elements known that have a naturally
FULL Valence Shell (Outer energy level) Since nonreactive, then they will
ALWAYS be found FREE in nature and NEVER in a compound.
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Periodic Table e- configuration from the periodic table
(To be covered in future chapters)
B2p1
1IA
18VIIIA
12
IIA13
IIIA14
IVA15VA
16VIA
17VIIA
2
33
IIIB4
IVB5
VB6
VIB7
VIIB8 9
VIIIB10 11
IB12IIB
4
5
6
7
H1s1
Li2s1
Na3s1
K4s1
Rb5s1
Cs6s1
Fr7s1
Be2s2
Mg3s2
Ca4s2
Sr5s2
Ba6s2
Ra7s2
Sc3d1
Ti3d2
V3d3
Cr4s13d5
Mn3d5
Fe3d6
Co3d7
Ni3d8
Zn3d10
Cu4s13d10
B2p1
C2p2
N2p3
O2p4
F2p5
Ne2p6
He1s2
Al3p1
Ga4p1
In5p1
Tl6p1
Si3p2
Ge4p2
Sn5p2
Pb6p2
P3p3
As4p3
Sb5p3
Bi6p3
S3p4
Se4p4
Te5p4
Po6p4
Cl3p5
Be4p5
I5p5
At6p5
Ar3p6
Kr4p6
Xe5p6
Rn6p6
Y4d1
La5d1
Ac6d1
Cd4d10
Hg5d10
Ag5s14d10
Au6s15d10
Zr4d2
Hf5d2
Rf6d2
Nb4d3
Ta5d3
Db6d3
Mo5s14d5
W6s15d5
Sg7s16d5
Tc4d5
Re5d5
Bh6d5
Ru4d6
Os5d6
Hs6d6
Rh4d7
Ir5d7
Mt6d7
Ni4d8
Ni5d8
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Summary
Periodic Table: Map of the Building block of matter
Type: Metal, metalloid and Nonmetal
Groupings: Representative or main, transition and Lanthanide/Actinides (rare)
Family: Elements in the same column have similar chemical property because of similar valence electrons
Alkali Metal, Alkaline Earth Metal, halogens, noble gases
Period: Elements in the same row have valence electrons in the same shell.
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Iron Triad
Iron (Fe)Cobalt
(Co)Nickel
(Ni)
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Coinage Elements
Copper (Cu)
Silver (Ag)
Gold (Au)
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Liquid @ Room Temp
Mercury (Hg) and Bromine (Br)