organization of the periodic table. columns of the periodic table atoms of elements in the same...
TRANSCRIPT
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Periodic TrendsOrganization of the Periodic Table
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GROUPS
Columns of the periodic table Atoms of elements in the same
group have the same # of valence electrons and therefore behave similarly
PERIODS•Rows of the periodic table•All elements in a period have their valence electrons in the same energy level.
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Which of the following are in the same group?
H, H
e, C, L
i
K, Ca, A
s, Br
He, N
e, Kr,
Ar
B, Al, G
e, Sn
0% 0% 0% 0%
1. H, He, C, Li2. K, Ca, As, Br3. He, Ne, Kr, Ar4. B, Al, Ge, Sn
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Which of the following are in the same period?
H, H
e, C, L
i
K, Ca, A
s, Br
He, N
e, Kr,
Ar
B, Al, G
e, Sn
0% 0% 0% 0%
1. H, He, C, Li2. K, Ca, As, Br3. He, Ne, Kr, Ar4. B, Al, Ge, Sn
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Representative and Transition Elements
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Valence Electrons Valence Electrons are electrons in the
outermost energy level.
- s or p electrons only (even when d and f electrons are present they are not in the outermost energy level)
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Electron Dot Diagrams Electron Dot Diagrams show the valence
electrons of an element.
Draw the electron dot diagrams for the following:
Mg N F
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How many valence electrons are in the halogens?
1 2 7 8
0% 0% 0% 0%
1. 12. 23. 74. 8
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How many valence electrons are in Group 17?
1 2 7 8
0% 0% 0% 0%
1. 12. 23. 74. 8
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How many valence electrons are in zinc and chromium?
1 2 7 8
Unable to
tell
0% 0% 0% 0% 0%
1. 12. 23. 74. 85. Unable to tell
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Size of the Atom Think of a ball of an onion. What happens
with each layer?
As you go down the periodic table, the energy levels increase and the size of the radius of the atom increases. (each energy level is like another layer of the onion)
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Which element has a larger atomic radius: Na or K?
Na K
Unable to
be determ
ined
0% 0% 0%
1. Na2. K3. Unable to be
determined
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Which element has a larger atomic radius: Br or Cl?
Br Cl
Unable to
be determ
ined
0% 0% 0%
1. Br2. Cl3. Unable to be
determined
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Atomic Radius cont.
• As you move from left to right in the periodic table, what happens to the number of protons in the nucleus?
• What effect do these protons have on the electrons?
• What effect do the electrons have on each other?
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Electron Shielding
• Electron Shielding (or Screening) – These inner electrons shield the valence electrons from receiving the entire attractive nuclear charge because they repel the valence electrons.
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Nuclear Charge and Atomic Radius Within a period, as you go from left to right,
the positive nuclear charge increases, and attracts the electrons more strongly.
As the electrons are more attracted to the nucleus, the atomic radius decreases.
Summary: as you go from left to right, the atomic radius generally decreases.
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Which element has a larger atomic radius: Li or Be?
Li Be
Unable to
be determ
ined
0% 0% 0%
1. Li2. Be3. Unable to be
determined
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Which element has a larger atomic radius: Si or Ar?
Si A
r
Unable to
be d...
0% 0% 0%
1. Si2. Ar3. Unable to be
determined
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Which element has a larger atomic radius: Be or Mg?
Be M
g
Unable to
be d...
0% 0% 0%
1. Be2. Mg3. Unable to be
determined
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Which element has a larger atomic radius: Si or C?
C Si
Unable to
be d...
0% 0% 0%
1. C2. Si3. Unable to be
determined
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Octet Rule The octet rule states that all atoms
attempt to become stable by having a full valence electron shell (generally 8 electrons, hence octet rule).
Atoms will gain, lose, or share electrons in order to attain this stability.
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Which group already has a full octet?
Alkali m
etals
Transiti
on met..
.
Halogens
Noble G
ases
0% 0% 0% 0%
1. Alkali metals2. Transition metals3. Halogens4. Noble Gases
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Which group is one electron away from a full octet?
14% 14% 14% 14% 14% 14% 14%1. Alkali metals2. Transition metals3. Halogens4. Alkaline earth
metals5. Both alkali metals
and halogens6. Noble gases7. Both alkali metals
and alkaline earth metals
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Ionization Energy Electrons are held in atoms by their
attraction to the positively charged nucleus.
To remove an electron requires energy.
Ionization energy is the energy required to remove the least tightly bound (or outermost) electron from an atom.
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Ionization Energy cont. Compare Li and K.
How many valence electrons?
What is the relative size of the atoms?
Which has a higher ionization energy?
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Ionization Energy As you go down a group, the ionization
energy decreases because it takes less energy to remove an electron.
The least tightly bound electrons are further from the positive nucleus, and can therefore be removed more easily.
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Which group has a higher ionization energy?
Halogens
Alkali M
etals
Alkalin
e Earth M
etals
All t
he same
0% 0% 0% 0%
1. Halogens2. Alkali Metals3. Alkaline Earth
Metals4. All the same
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Which element has a higher ionization energy?
Li Be F Ne
0% 0% 0% 0%
1. Li2. Be3. F4. Ne
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Which element has the lowest ionization energy?
Na
Mg S A
r
0% 0% 0% 0%
1. Na2. Mg3. S4. Ar
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Summary Ionization energy generally decreases as
you go down a group and from right to left in a period.
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Ionization energy
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A Quick Review …
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How many valence electrons does oxygen have?
1 3 4 6 8
0% 0% 0% 0% 0%
1. 12. 33. 44. 65. 8
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Which has the biggest atomic radius?
K Na Li Be Cs
Ca F
0% 0% 0% 0% 0% 0% 0%
1. K2. Na3. Li4. Be5. Cs6. Ca7. F
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What is the effective nuclear charge on lithium?
1 2 3
None of t
he ab...
0% 0% 0% 0%
1. 12. 23. 34. None of the above
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Which has the greatest ionization energy?
K Na Li Be Cs
Ca F
0% 0% 0% 0% 0% 0% 0%
1. K2. Na3. Li4. Be5. Cs6. Ca7. F
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How many valence electrons are in group 14?
1 4 7 14
0% 0% 0% 0%
1. 12. 43. 74. 14
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Second, Third, etc. Ionization Energy Second ionization is the energy required to
remove a second electron. Ex. Sodium has a lower (first) ionization
energy than Magnesium but Mg has a lower second ionization energy than Na.
Why?
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Which has a lower third ionization energy?
K Ca G
a C
0% 0% 0% 0%
1. K2. Ca3. Ga4. C
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Electronegativity Electronegativity is the tendency of an
element to attract electrons in a bond.
Therefore, elements that want to gain electrons will have higher electronegativity.
attractive
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Which group of elements is most likely to gain electrons to become stable?
Alkali M
etals
Transiti
on Met..
.
Halogens
Noble G
ases
0% 0% 0% 0%
1. Alkali Metals2. Transition Metals3. Halogens4. Noble Gases
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Which has the greatest electronegativity?
K Na Li Be Cs
Ca F
0% 0% 0% 0% 0% 0% 0%
1. K2. Na3. Li4. Be5. Cs6. Ca7. F
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Which group has the lowest electronegativity (not counting noble gases)?
Alkali m
etals
Alkalin
e earth...
Halogens
Transiti
on Met..
.
0% 0% 0% 0%
1. Alkali metals2. Alkaline earth
metals3. Halogens4. Transition Metals
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Trend Summaries
The pattern forincreasing electronegativity(except for noble gases).
The pattern for increasing ionization energy.
The pattern for increasingatomic radius.
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Ions When an atom loses or gains electrons, it
gains a charge. An ion is a charged atom.
A positive ion is called a cation. (ex. Na+)
A negative ion is called an anion. (ex. S2-)
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Size of Ions Cations (positive) – lose valence electrons in
the outermost energy level.◦ They lose an energy level so they get smaller.
Anions (negative) – gain valence electrons but their Zeff does not change.◦ They get bigger because of having more electrons
and the same Zeff
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Which is a bigger atom?
Mg
Mg+
Mg2+
0% 0% 0%
1. Mg2. Mg+
3. Mg2+
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Which is a bigger atom?
O O-
O2-
0% 0% 0%
1. O2. O-
3. O2-
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Which is a bigger atom?
Ca Ca+
Ca2+
0% 0% 0%
1. Ca2. Ca+
3. Ca2+
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Which is a bigger atom?
S S- S2-
0% 0% 0%
1. S2. S-
3. S2-
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Cations Groups 1-13 become cations by losing
electrons because of their low ionization energy.
Their positive charge corresponds to their group number.
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Anions Groups 15-17 become anions by gaining
electrons because of their high electronegativity.
Their negative charge corresponds to how many electrons they must gain to have the same electron configuration as a noble gas.
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Which of the following describes the tendency for an element to attract an electron in a bond?
Ioniza
tion energy
Ato
mic ra
dius
Thermal c
apacity
Electronegativity
0% 0% 0% 0%
1. Ionization energy2. Atomic radius3. Thermal capacity4. Electronegativity
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Which of the following elements is most likely to carry a +2 charge as a cation?
Aluminum
Oxy
gen
Magnesiu
m
Lith
ium
0% 0% 0% 0%
1. Aluminum2. Oxygen3. Magnesium4. Lithium
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If an element has a high electronegativity it also has a large:
Ato
mic ra
dius
Ioniza
tion Energy
Ato
mic M
ass
Ionic
Charge
0% 0% 0% 0%
1. Atomic radius2. Ionization Energy3. Atomic Mass4. Ionic Charge
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4 Different kinds of metals◦ Alkali metals: soft, shiny and very reactive
Group 1: not found in nature as elements◦ Alkaline earth-metals: less reactive
Group 2: have two valence electrons◦ Transition Metals: many uses
Groups 3-12
METALS
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3 Different kinds of metals◦ Noble Gases: mostly non-reactive, very stable
Group 8: He, Ne, Ar, Kr, Xe, Rn◦ Halogens: very reactive, gain one electron to
form a stable compound Group 7: F, Cl, Br, I
NONMETALS
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Seven elements are called diatomic and never exist alone in nature.
Have No Fear Of Ice Cold Beans????? H2
N2
F2
O2
I2 Cl2 Br2
Diatomic Gases
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Magnesium is in which group?
Alkali m
etals
Alkalin
e earth...
Transiti
on met..
.
Halogens
Noble gase
s
0% 0% 0% 0% 0%
1. Alkali metals2. Alkaline earth
metals3. Transition metals4. Halogens5. Noble gases
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Lithium is in which group?
Alkali m
etals
Alkalin
e earth...
Transiti
on met..
.
Halogens
Noble gase
s
0% 0% 0% 0% 0%
1. Alkali metals2. Alkaline earth
metals3. Transition metals4. Halogens5. Noble gases
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Manganese is in which group?
Alkali m
etals
Alkalin
e earth...
Transiti
on met..
.
Halogens
Noble gase
s
0% 0% 0% 0% 0%
1. Alkali metals2. Alkaline earth
metals3. Transition metals4. Halogens5. Noble gases
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Krypton is in which group?
Alkali m
etals
Alkalin
e earth...
Transiti
on met..
.
Halogens
Noble gase
s
0% 0% 0% 0% 0%
1. Alkali metals2. Alkaline earth
metals3. Transition metals4. Halogens5. Noble gases
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The majority of the diatomic gases are in which group?
Alkali m
etals
Alkalin
e earth...
Transiti
on met..
.
Halogens
Noble gase
s
0% 0% 0% 0% 0%
1. Alkali metals2. Alkaline earth
metals3. Transition metals4. Halogens5. Noble gases
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Metals◦Shiny ◦Solids◦Stretched and
Shaped◦Conductors of
heat and electricity
Nonmetals◦Solids, liquids or
gases◦Solids – dull and
brittle◦Poor conductors of
heat and electricity
****Semiconductors / Metalloids – exhibit properties of both metals and nonmetals
FAMILIES OF ELEMENTS
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Metals◦ On the left hand side of
the zigzag line (except for Hydrogen – exception)
- Metalloids or Semi-metals- Touching zigzag line (Except for Al)- Exhibit properties of both metals and nonmetals
Nonmetals◦ On the right hand
side of the zig zag line (plus Hydrogen)
How do you tell if it’s a metal, nonmetal, or metalloid?
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The difference in electronegativity between atoms A and B is given by: