Standards 2 & 10 Review
Name:______________________________
Date: _____________________ Period:___
2.0 Chemical Bonds: Biological, chemical, and physical properties of matter result from the ability of
atoms to form bonds from electrostatic forces between electrons and protons and between atoms and
molecules. As a basis for understanding this concept:
a. Students know atoms combine to form molecules by sharing electrons to form covalent bonds,
delocalized electrons to form metallic bonds, or by exchanging electrons to form ionic bonds.
1. Potassium (K) and chlorine (Cl) form a(n):
a. Covalent bond.
b. Hydrogen bond.
c. Ionic bond.
d. Metallic bond.
2. When atoms combine to form a molecule by sharing electrons, what types of bonds are formed?
a. Covalent bond
b. Hydrogen bond
c. Ionic bond
d. Metallic bond
3. Which is the best way to express the relationship between hydrogen and fluorine when they
combine?
a.
b.
c.
d.
4. A metallic bond is formed between:
a. A metal atom and a hydrogen atom.
c. A metal atom and a noble gas.
b. A metal atom and a nonmetallic atom.
d. Two metal atoms.
5. A scientist discovers a new compound. After chemical testing, the compound is found to have a
high melting point and high boiling point. What type of bond holds the compound together?
a. Ionic
b. covalent
c. metallic
d. polar
6. Which of the following is not a property of metals?
a. Malleability
b. ductility
c. brittle
d. shiny
b. Students know chemical bond between atoms in molecules such as H2, CH4, NH3, H2CCH2, N2, Cl2, and
many large biological molecules are covalent.
7. Which do not form covalent bonds?
a. Diatomic molecules b. Large biological molecules c. Molecules containing carbon d. Salts
8. The bonds found in C2H4 are:
a. Non-Polar Covalent
b. Ionic
c. Metallic
d. Polar Covalent
9. Which is a covalent compound?
a. AlBr3
b. CO2
c. KCl
d. NaF
10. Which is a covalent compound?
a. Mg3N2
b. NaCl
c. NaF
d. SiF4
11. Which is not a covalent compound?
a. CCl4
b. H2
c. MgCl2
d. SO3
12. Some of the molecules found in the human body are NH2CH2COOH (glycine), and C6H12O6
(glucose). The bonds they form are:
a. Nuclear
b. metallic
c. ionic
d. covalent
c. Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions
d. Students know the atoms and molecules in liquids move in a random pattern relative to one another
because the intermolecular forces are too weak to hold the atoms or molecules in solid form.
h.* Students know how to identify solids and liquids held together by Van der Waals forces or hydrogen
bonding and relate these forces to volatility and boiling/melting point temperatures.
13. At room temperature, which substance has the weakest intermolecular forces?
a. Oxygen gas
b. Salt
c. Steel
d. Uranium
14. This state of matter occurs when there is no amount of intermolecular attraction between
molecules.
a. Solid
b. Liquid
c. Gas
d. Plasma
15. Which of the following shows increasing intermolecular forces (as read from the left to the right)?
a. Solid, gas, liquid
b. Solid, liquid, gas c. Gas, liquid, solid d. Liquid, gas, solid
16. A molecule of F2 gas is held together by:
a. Polar covalent bond b. non-polar covalent bond c. ionic bond
d. metallic bond
17. Which of the following will have the strongest intermolecular forces?
a. HF
b. CH4
c. NaCl
d. Cu
18. Electrons involved in a polar covalent bond are:
a. Transferred
b. shared equally
d. overlapped
c. shared unequally
19. Which statement best explains why CH4 is a non-polar molecule?
a. CH4 has a symmetrical charge distribution
b. C and H are non-metals
c. C and H have the same electronegativity
d. CH4 has four bonds.
20. Compared to intramolecular bonds, the strength of intermolecular forces are:
a. Weaker
b. Stronger
c. About the same strength d. Unknown
e. Students know how to draw Lewis dot structures.
g.* Students know how electronegativity and ionization energy relate to bond formation.
21. Which of the following has the same Lewis Dot structure as germanium?
a. Si
b. Al
c. As
d. Ga
22. The tendency of an atom to attract electrons to itself when it is bonded to another atom is:
a. Electronegativity b. ionization energy
c. electron affinity d. electrostatic repuslion
10.0 Organic Chemistry & Biochemistry: The bonding characteristics of carbon allow the formation
of many different organic molecules of varied sizes, shapes, and chemical properties and provide
the biochemical basis of life. As a basis for understanding this concept:
a. Students know large molecules (polymers), such as proteins, nucleic acids, and starch, are formed
by repetitive combinations of simple subunits.
b. Students know amino acids are the building blocks of proteins.
23. Proteins are large macromolecules composed of thousands of subunits. The structure of the
protein depends on the sequence of:
a. Lipids
b. monosacharides (sugars) c. amino acids
d. nucleosides
24. Nucleic acids are polymers whose structure depends on the sequence of:
a. Sugar
b. nitrogen base
c. phosphate
d. all of the above