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Chemistry
10th -
12thgrade
Holt Modern Chemistry Chapter 6 Review
62 questions
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- 1. Multiple Choice
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- 11. Multiple Choice
Ionic bonds form as a result of the electrostatic attraction between:
Dipoles
Electrons
Ions
Nuclei
- 12. Multiple Choice
A single covalent bond involves the sharing of:
Only one electron
Two electrons
Three electrons
A variable number of electrons which depends on the bonding atoms.
- 13. Multiple Choice
Na and Cl
O and Cl
H and O
Na and O
None of the given answers
- 14. Multiple Choice
K and N
K and S
N and Br
S and Br
None of the given answers
- 15. Multiple Choice
A measure of an atoms ability to attract electrons is:
Electronegativity
Polarization
Ionization
Electron Affinity
Both polarization and ionization
- 16. Multiple Choice
Atoms that are bonded with an electronegativity difference of 0 to 0.3 are generally considered to be:
Negatively charged compounds
Non-polar covalent compounds
Polar covalent compounds
Ionic compounds
Diatomic compounds
- 17. Multiple Choice
What is the apparent charge on the chlorine atom in the HCl molecule?
+1
-1
- 18. Multiple Choice
Atoms seldom exist as independent particles in nature because:
as single particles, most atoms have low potential energy
their electronegativity is much lower when they combine with other atoms
atoms are more stable when they combine with other atoms
neutral particles are very rare.
- 19. Multiple Choice
When an atom completely gives up its valence electrons to another atom, they form a bond that is considered to be:
Purely ionic
Partially ionic
Polar-covalent
Nonpolar-covalent
Not a bond
- 20. Multiple Choice
You can estimate the degree to which a bond between two atoms is ionic or covalent by calculating the:
distance between atoms nuclei
difference in the atoms' electronegativities
atoms' atomic radii
number of atoms in the compound
overall atomic mass
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- 41. Multiple Choice
If two covalently bonded atoms move closer than a distance of the bond length, the potential energy of the atoms:
becomes negative
decreases
increases
remains constant
halves
- 42. Multiple Choice
The electrons involved in the formation of a covalent bond are:
transferred from one atom to another
found only in the s orbitals
valence electrons
in filled orbitals
- 43. Multiple Choice
Bond energy is the energy
absorbed as a molecule forms
change as atoms get closer together
required to break a chemical bond and form separate, neutral atoms
of two covalently bonded atoms.
- 44. Multiple Choice
Bond length between two bonded atoms is:
twice the diameter of the molecular orbital
the separation at which their potential energy is minimum
the separation at which the motion of each atom stops
the sum of the diameters of each of the two overlapping electron clouds
- 45. Multiple Choice
Which compound most likely has the greatest bond energy?
HF; H-F bond length = 92 pm
I2; I-I bond length = 266 pm
Cl2; Cl-Cl bond length = 199 pm
HCl; H-Cl bond length = 127 pm
- 46. Multiple Choice
The Lewis Structure of which of the following compounds does not follow the octet rule?
NH3
BF3
CCl4
H2O
- 47. Multiple Choice
In a double covalent bond,
one atom has more than eight valence electrons
one atom loses a pair of electrons
two atoms share eight valence electrons
two atoms share two pairs of electrons
- 48. Multiple Choice
Which of the following is NOT a resonance structure of SO3?
- 49. Multiple Choice
How many double bonds are in the Lewis structure for hydrogen fluoride, HF?
None
One
Two
Three
Impossible to tell
- 50. Multiple Choice
To draw a Lewis structure, it is NOT necessary to know:
The length of the bonds
The types of atoms in the molecule
The number of valence electrons for each atom
The number of atoms in the molecule
- 51. Multiple Choice
Determine the molecular geometry of the given structure.
Trigonal Pyramidal
Trigonal Bipyramidal
Trigonal Planar
Tetrahedral
- 52. Multiple Choice
The geometry of a molecule with 4 bonded pairs of electrons and 0 lone pairs of electrons, AB4
Tetrahedral
Trigonal Planar
Bent
Trigonal Pyramidal
Linear
- 53. Multiple Choice
The geometry of a molecule with 2 bonded pairs of electrons and 2 lone pairs of electrons, AB2E2
Tetrahedral
Trigonal Planar
Bent
Trigonal Pyramidal
Linear
- 54. Multiple Choice
The geometry of a molecule with 3 bonded pairs of electrons and 0 lone pairs of electrons, AB3
Tetrahedral
Trigonal Planar
Bent
Trigonal Pyramidal
Linear
- 55. Multiple Choice*lineartrigonal planartrigonal pyramidbent of angular
- 56. Multiple Choice*trigonal pyramidlinearbentangular
- 57. Multiple ChoiceSiCl4 has what shape?square planarsquare pyramidaltetrahedraloctahedral
- 58. Multiple ChoiceWhat is the shape of H2O?lineartetrahedralbenttrigonal pyramidal
- 59. Multiple ChoiceAccording to the octet rule most elements need _______ valence electrons.28618
- 60. Multiple Choice
What is the molecular geometry of CO2?
Bent
Trigonal planar
Trigonal pyramidal
Linear
- 61. Multiple ChoiceDiagram below showsformation of hybrid orbitalatomic orbital overlap to produce hybrid orbitalatomic orbital overlap to form sp hybrid orbitals orbital overlap with p orbital to form sp hybrid orbital
- 62. Multiple ChoiceWhich of the statement is TRUE?s orbital overlap with p orbitals to form sp hybrid orbitals orbital with two p orbitals to form one sp2 hybrid orbitals orbital with two p orbitals to form two sp2 hybrid orbitals orbital with two p orbitals to form three sp2 hybrid orbital
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