Ch. 8 Covalent Compounds Question Preview (ID: 35956)
This Test Covers Covalent Bonding, Lewis Structures, VSPER Theory, And Electronegativity Differences.
TEACHERS: click here for quick copy question ID numbers.
Covalent compounds result from atoms
a) transferring electrons.
b) sharing electrons.
c) splitting into smaller atoms.
d) sharing protons.
In what form do diatomic elements normally occur?
a) a single atom?
b) as molecules containing two atoms
c) as molecules containing three atoms
d) as molecules containing 4 atoms
How many electrons are shared in a double covalent bond?
a) 1
b) 2
c) 3
d) 4
Which of the following is a property of molecular compounds?
a) good conductors at room temperature
b) always a solid at room temperature
c) made of cations and anions that are attracted to each other
d) can be a solid, liquid, or gas at room temperature
Resonance occurs when
a) there is not Lewis structure to accurately represent the arrangements of atoms in a molecule.
b) there are multiple multiple Lewis structures to accurately represent the arrangement of atoms in a molecule.
c) the Lewis structure of a molecule has a central atom with an incomplete octet.
d) the Lewis structure of the molecule has a central atom with an expanded octet.
CH4 (the 4 should be a subscript but the website will not allow it) is an example of
a) molecular formula.
b) structural formula.
c) formula unit.
d) none of the above.
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) add the ion charge to
d) none of the above.
In general,
a) the fewer the electron pairs that are shared, the stronger the bond.
b) the more electron pairs that are shared, the stronger the bond.
c) triple bonds are longer than single bonds.
d) the number of electrons shared has no effect on length or strength of a bond.
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.
Which of the following elements is NEVER a central atom of a Lewis structure
a) carbon
b) nitrogen
c) hydrogen
d) phosphorus
How many covalent bonds do group 15 elements generally form?
a) 1
b) 2
c) 3
d) 4
How many covalent bonds do group 17 elements (halogens) generally form?
a) 1
b) 2
c) 3
d) 4
A covalent bonds forms between
a) the nuclei of one atom and its electrons
b) the nuclei of one atom and the nuclei 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 electrons of a nearby atom
A molecular compound consists of
a) at least 2 nonmetals bonded together.
b) a metal and a nonmetal atoms.
c) both a and b can be a molecular compound.
d) none of the above.
The VSEPR theory allows us to predict
a) the polarity of molecules.
b) the size of molecules.
c) the shape of molecules.
d) the melting point of molecules.
The VSEPR theory is based on the general idea that
a) the negatively charged electrons will repel each other in molecules, to create a specific shapes.
b) the shapes of molecules are random and unpredictable.
c) the shapes of molecules are due to the nuclei of adjacent atoms repelling each other.
d) the sharing of valence electrons is unequal.
Which of the following elements is most likely to be the central atom of a Lewis structure?
a) carbon
b) helium
c) fluorine
d) oxygen
Which of the following is the best rule to determine which element will be a central atom
a) the atom with the highest electronegativity will always be a central atom.
b) the atom with the lowest electronegativity will be a central atom.
c) the atom that is written first is usually the central atom.
d) if there is only one of that atom it is may be a central atom.
What term is given to the amount of control an atom has over bonded electrons?
a) electron affinity
b) polarity
c) ionization energy
d) electronegativity
The type of bond formed between two elements can be determined using
a) differences in ionization energies.
b) molecular geometry.
c) electronegativity differences.
d) VSEPR theory.
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