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Ch. 8 Covalent Compounds
Test Description: This test covers covalent bonding, Lewis structures, VSPER theory, and electronegativity differences.
Instructions: Answer all questions to get your test result.
1) Covalent compounds result from atoms
A
sharing protons.
B
splitting into smaller atoms.
C
sharing electrons.
D
transferring electrons.
2) In what form do diatomic elements normally occur?
A
as molecules containing two atoms
B
a single atom?
C
as molecules containing three atoms
D
as molecules containing 4 atoms
3) How many electrons are shared in a double covalent bond?
A
4
B
1
C
3
D
2
4) Which of the following is a property of molecular compounds?
A
can be a solid, liquid, or gas at room temperature
B
made of cations and anions that are attracted to each other
C
good conductors at room temperature
D
always a solid at room temperature
5) Resonance occurs when
A
the Lewis structure of the molecule has a central atom with an expanded octet.
B
the Lewis structure of a molecule has a central atom with an incomplete octet.
C
there are multiple multiple Lewis structures to accurately represent the arrangement of atoms in a molecule.
D
there is not Lewis structure to accurately represent the arrangements of atoms in a molecule.
6) CH4 (the 4 should be a subscript but the website will not allow it) is an example of
A
formula unit.
B
molecular formula.
C
structural formula.
D
none of the above.
7) When writing the Lewis structure for a positive polyatomic ion, you should _______________ the total number of valence electrons available for bonding.
A
subtract the ion's charge from
B
not use the ion's charge to change
C
none of the above.
D
add the ion charge to
8) In general,
A
the fewer the electron pairs that are shared, the stronger the bond.
B
the number of electrons shared has no effect on length or strength of a bond.
C
the more electron pairs that are shared, the stronger the bond.
D
triple bonds are longer than single bonds.
9) Bond dissociation measures
A
the amount of energy required to form a covalent bond.
B
the energy required to break a covalent bond.
C
the amount of energy required to separate a crystal lattice.
D
the amount of energy required to forma crystal lattice.
10) Which of the following elements is NEVER a central atom of a Lewis structure
A
carbon
B
phosphorus
C
hydrogen
D
nitrogen
11) How many covalent bonds do group 15 elements generally form?
A
4
B
1
C
2
D
3
12) How many covalent bonds do group 17 elements (halogens) generally form?
A
4
B
1
C
2
D
3
13) A covalent bonds forms between
A
the nuclei of one atom and its electrons
B
the nuclei of one atom and the electrons of a nearby atom
C
the electrons of one atom and the electrons of a nearby atom
D
the nuclei of one atom and the nuclei of a nearby atom
14) A molecular compound consists of
A
none of the above.
B
both a and b can be a molecular compound.
C
a metal and a nonmetal atoms.
D
at least 2 nonmetals bonded together.
15) The VSEPR theory allows us to predict
A
the polarity of molecules.
B
the shape of molecules.
C
the size of molecules.
D
the melting point of molecules.
16) The VSEPR theory is based on the general idea that
A
the shapes of molecules are due to the nuclei of adjacent atoms repelling each other.
B
the sharing of valence electrons is unequal.
C
the negatively charged electrons will repel each other in molecules, to create a specific shapes.
D
the shapes of molecules are random and unpredictable.
17) Which of the following elements is most likely to be the central atom of a Lewis structure?
A
oxygen
B
carbon
C
fluorine
D
helium
18) Which of the following is the best rule to determine which element will be a central atom
A
the atom that is written first is usually the central atom.
B
if there is only one of that atom it is may be a central atom.
C
the atom with the lowest electronegativity will be a central atom.
D
the atom with the highest electronegativity will always be a central atom.
19) What term is given to the amount of control an atom has over bonded electrons?
A
ionization energy
B
electron affinity
C
polarity
D
electronegativity
20) The type of bond formed between two elements can be determined using
A
electronegativity differences.
B
differences in ionization energies.
C
VSEPR theory.
D
molecular geometry.
*select an answer for all questions
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