Question 1
Choose the member of each set that best matches the label.
More covalent N2O, Na2O
Highest electronegativity O, S, Br
1. N2O, Br
2. N2O, O
3. Na2O, S
4. Na2O, O
5. Na2O, Br
2.
Question 2
Which of the following bonds would be the most polar without being considered ionic?
1. Mg-O
2. C-O
3. O-O
4. Si-O
5. N-O
3.
Question 3
Which of the following compounds contains one or more covalent bonds?
1. SO2
2. NaBr
3. Rb2O
4. MgBr2
5. MgO
4.
Question 4
Would NaBr be classified as ionic or covalent?
Question 5
Rank the following bonds from least polar to most polar:
Si-Cl, P-Cl, Mg-Cl, and S-Cl
1. S-Cl < P-Cl < Mg-Cl < Si-Cl
2. P-Cl < S-Cl < Si-Cl < Mg-Cl
3. Mg-Cl < Si-Cl < P-Cl < S-Cl
4. Mg-Cl < S-Cl < P-Cl < Si-Cl
5. S-Cl < P-Cl < Si-Cl < Mg-Cl
Question 6
Which of the following elements has the lowest electronegativity?
6. Cs
7. Na
8. Be
9. Se
10. Br
Question 7
Draw the Lewis electron structure for the sulfur atom.
Question 8
Would SF4 be classified as ionic or covalent?
5.
Question 9
Write the electron configuration for Al3+.
Question 10
Which of the following molecules has a trigonal planar structure?
1. CH4
2. NO3-
3. CO2
4. CO
5. H2
6.
Question 11
Which of the following has primarily ionic bonding?
1. N2O3
2. Na2O
3. CO2
4. CCl4
5. none of these
7.
Question 12
True or false? Ionic bonding occurs between atoms with small differences in electronegativities.
8.
Question 13
Consider the molecule SO2. Answer the following.
What is the electron arrangement around the central atom?
9.
Question 14
A oxygen atom needs to gain _____ electrons to achieve a noble gas configuration.
1. 2
2. 1
3. 3
4. 4
5. 5
10.
Question 15
True or false? N2 is an example of a covalent bond.
11.
Question 16
Draw the Lewis structure for SiH4.
Question 17
Draw the Lewis electron structure for the Cl2 molecule.
12.
Question 18
Which of the following molecules has only nonpolar covalent bonds?
1. N2
2. CO
3. HI
4. CCl4
5. NaCl
13.
Question 19
Would K2O be classified as ionic or covalent?
14.
Question 20
Which of the following covalent molecules has a linear structure?
1. SO2
2. CO2
3. OF2
4. SCl2
5. NH2
15.
Question 21
Which has a trigonal pyramid structure?
1. SO32-
2. CO32-
3. SO3
4. NO3-
5. CH4
16.
Question 22
True or false? The F- and O2- ions have the same electron configuration.
Question 23
1 Point
This molecule contains a carbon atom with trigonal planar geometry.
1. CH3CHO
2. CO2
3. CH3Cl
4. C2H6
17.
Question 24
Use the following choices to describe the molecular structure of each of the following molecules or ions.
a. linear
b. trigonal planar
c. tetrahedral
d. pyramidal
e. V-shaped
OCl2
Question 25
Which element or ion listed below has the electron configuration 1s22s22p63s23p6?
1. S
2. Ne
3. Cl
4. S2-
5. none of these
18.
Question 26
Which of the following molecules has more than one reasonable resonance structure?
1. CH4
2. CO2
3. PH3
4. HF
5. HCl
19.
Question 27
Use the following choices to describe the molecular structure of each of the following molecules or ions.
a. linear
b. trigonal planar
c. tetrahedral
d. pyramidal
e. V-shaped
PF3
20.
Question 28
Which of the following element or ion has the electron configuration 1s22s22p63s23p6?
1. Cl
2. Br-
3. Se
4. Ca2+
5. Two of these
21.
Question 29
Draw the Lewis structure for CCl4.
Question 30
Consider the molecule SO2. Answer the following.
How many lone pairs of electrons are around the central atom?
31-Consider the following processes:
2ClF+O2-> Cl2O+F2O
167.4
2ClF3+2O2->Cl2O+3F2O
341.4
2F2+O2->2F2O
–43.4
Full Answer Section
Question 5
- S-Cl < P-Cl < Si-Cl < Mg-Cl
Question 6
Cs has the lowest electronegativity.
Question 7
Lewis electron structure for sulfur atom
Question 8
SF4 is a covalent compound.
Question 9
The electron configuration for Al3+ is 1s22s22p6.
Question 10
- NO3- has a trigonal planar structure.
Question 11
- Na2O has primarily ionic bonding.
Question 12
False. Ionic bonding occurs between atoms with large differences in electronegativities.
Question 13
The electron arrangement around the central atom (sulfur) in SO2 is trigonal pyramidal.
Question 14
- A oxygen atom needs to gain 2 electrons to achieve a noble gas configuration.
Question 15
True. N2 is an example of a covalent bond.
Question 16
Question 17
Lewis electron structure for Cl2 molecule
Additional Information
Electronegativity
Electronegativity is a measure of how strongly an atom attracts electrons. Atoms with higher electronegativities attract electrons more strongly than atoms with lower electronegativities.
Ionic Bonding
Ionic bonding occurs between atoms with large differences in electronegativities. In ionic bonding, one atom transfers one or more electrons to another atom. The atom that transfers electrons becomes a positively charged cation, and the atom that gains electrons becomes a negatively charged anion.
Covalent Bonding
Covalent bonding occurs between atoms with similar electronegativities. In covalent bonding, atoms share electrons to form a bond.
Lewis Structures
Lewis structures are a way of representing the valence electrons of atoms and molecules. Lewis structures can be used to predict the shape of molecules and to identify polar bonds.
Polar Bonds
A polar bond is a bond between two atoms with different electronegativities. In a polar bond, the electrons are not shared equally between the two atoms. The atom with the higher electronegativity has a greater share of the electrons.
Nonpolar Bonds
A nonpolar bond is a bond between two atoms with the same electronegativity. In a nonpolar bond, the electrons are shared equally between the two atoms.
Molecular Structure
The molecular structure of a molecule is the arrangement of its atoms in space. The molecular structure of a molecule is determined by the number of valence electrons on each atom and the electronegativities of the atoms.