lectureplus timberlake1 chemical bonds attraction between two or more atoms interaction between...
TRANSCRIPT
LecturePLUS Timberlake 1
Chemical Bonds
Attraction between two or more atomsInteraction between valence electronsIonic bondsCovalent bonds
LecturePLUS Timberlake 2
Valence Electrons
Electrons in the highest (outer) electron level
Have most contact with other atoms
Known as valence electrons
Outer shelI of noble gases the outer shell
contains 8 valence electrons as s2p6 (except
He = 2)
Example: Ne 1s2 2s2 2p6
Ar 1s2 2s2 2p6 3s2 3p6
LecturePLUS Timberlake 3
Electron Dot Structures
Symbols of atoms with dots to represent the valence-shell electrons
1A 2A 3A 4A 5A 6A 7A 8A
H He: Li Be B C N O : F : Ne :
Na Mg Al Si P S : Cl : Ar :
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Learning Check B1
A. X would be the electron dot formula for
1) Na 2) K 3) Al
B. X would be the electron dot formula
1) B 2) N 3) P
LecturePLUS Timberlake 5
Solution B1
A. X would be the electron dot formula for
1) Na 2) K
B. X would be the electron dot formula
2) N 3) P
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Octet Rule
An octet in the outer shell makes atoms stable
Electrons are lost, gained or shared to form an octet
Unpaired valence electrons strongly influence
bonding
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Formation of Ions from Metals
• Ionic compounds result when metals react with
nonmetals
• Metals lose electrons to match the number of
valence electrons of their nearest noble gas
• Positive ions form when the number of
electrons are less than the number of protons
Group 1A metals ion 1+
Group 2A metals ion 2+
• Group 3A metals ion 3+
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Formation of Sodium Ion
Sodium atom Sodium ion
Na – e Na +
1s22s22p63s1 1s22s22p6 ( = Ne)
11 p+ 11 p+
11 e- 10 e-
0 1+
LecturePLUS Timberlake 9
Formation of Magnesium Ions
Magnesium atom Magnesium ion
Mg – 2e Mg2+
1s22s22p63s2 1s22s22p6 (Ne)
12 p+ 12 p+
12 e- 10 e-
0 2+
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Cations of Some Representative Elements
Group 1A Group 2A Group 3AH+ Mg2+ Al3+
Li+ Ca2+
Na+ Sr2+
K+ Ba2+
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Learning Check B 2
A. Number of valence electrons in aluminum1) 1 e- 2) 2 e- 3) 3 e-
B. Change in electrons for octet1) lose 3e- 2) gain 3 e- 3) gain 5 e-
C. Ionic charge of aluminum 1) 3- 2) 5- 3) 3+
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Solution B 2
A. Number of valence electrons in aluminum3) 3 e-
B. Change in electrons for octet1) lose 3e-
C. Ionic charge of aluminum 3) 3+
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Learning Check B 3
Give the ionic charge for each of the following:A. 12 p+ and 10 e-
1) 0 2) 2+3) 2-
B. 50p+ and 46 e-
1) 2+ 2) 4+3) 4-
C. 15 p+ and 18e-
2) 3+ 2) 3- 3) 5-
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Solution B 3
Give the ionic charge for each of the following:
A. 12 p+ and 10 e-
2) 2+
B. 50p+ and 46 e-
2) 4+
C. 15 p+ and 18e-
2) 3-
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Learning Check B 4
A. Why does Ca form a Ca2+ ion?
B. Why does O form O2- ion?
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Solution B 4
A. Why does Ca form a Ca2+ ion?
Loses 2 electrons to give octet
1s2 2s2 2p6 3s2 3p6 4s2
1s2 2s2 2p6 3s2 3p6 (like Ar)
B. Why does O form O2- ion?
Gains 2 electrons to give octet
1s2 2s2 2p4 + 2e-
1s2 2s2 2p6 2-8 (like Ne)
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Transition Metals
• Lose s electrons from the highest occupied
energy level.
• May also lose one or more d electrons.
• Most form 2 or more positive ions
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Fe2+ and Fe3+
Fe atom: 1s2 2s2 2p6 3s2 3p6 4s2 3d6
Loss of 4s2 electrons (outermost shell)
Fe2+ ion: 1s2 2s2 2p6 3s2 3p6 4s0 3d6
Loss of 3d1 electron
Fe3+ ion: 1s2 2s2 2p6 3s2 3p6 4s0 3d5
A 3d5 (half-filled) subshell is stable
LecturePLUS Timberlake 19
Some Transition Metal Ions
1+ 2+ 1+ or 2+ 2+ or 3+
Ag+ Cd2+ Cu+, Cu2+ Fe2+, Fe3+
silver cadmium copper(I) ion iron(II) ion
ion ion copper (II) ion iron(III) ion
Zn2+
zinc ion
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Ions from Nonmetal Ions
In ionic compounds, nonmetals in 5A, 6A,
and 7A gain electrons from metals
Nonmetal add electrons to achieve the octet
arrangement
Nonmetal ionic charge:
3-, 2-, or 1-
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Fluoride Ions
unpaired electron octet
1 -
: F + e : F :
1s22s22p5 1s22s22p6 = Ne
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Some Nonmetal Ions 5A 6A 7A
N3 O2 F
nitride __________ fluoride
P3 S2 Cl
___________ __________ _________
Br
_________
I
iodide ion
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Some Nonmetal Ions
5A 6A 7A
N3 O2 F
nitride oxide fluoride
P3 S2 Cl
phosphide sulfide chloride
Br
bromide
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Ionic Compounds
Attraction between + ions and - ions
Electrons go from metals to nonmetals
electron transfer
metal nonmetal ion+ ion-–
Electrons lost = Electrons gain
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Formulas of Ionic Compounds
Formulas of ionic compounds are determined from the charges on the ions
atoms ions
–
Na + F : Na+ : F : NaF
sodium fluorine sodium fluoride formula
Charge balance: 1+ 1- = 0
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Writing a Formula
Write the formula for the ionic compound that will form between Ba2+ and Cl.
Solution:
1. Balance charge with + and – ions
2. Write the positive ion of metal first, and the
negative ion Ba2+ Cl
Cl3. Write the number of ions needed as
subscripts BaCl2
LecturePLUS Timberlake 27
Learning Check B 5
A. The formula for the ionic compound of
Na+ and O2- is
1) NaO 2) Na2O 3) NaO2
B. The formula of a compound of aluminum and chlorine is
1) Al3Cl 2) AlCl2 3) AlCl3
C. The formula of Fe3+ and O2- is
1) Fe3O2 2) FeO3 3) Fe2O3