Name: Period: Date:

Chemistry

Review #3: Ionic, Covalent, Metallic Bonding

Standards to be mastered:

1.  Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds.

2.  Students know chemical bonds between atoms in molecules such as H2, CH4 , NH3 , H2 CCH2 , N2 , Cl2, and many large biological molecules are covalent.

3.  Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction.

4.  Students know the atoms and molecules in liquids move in random patterns relative to one another because intermolecular bonds are too weak to hold molecules in a solid form.

BOND:

1.  Intramolecular bond:

Ionic
Covalent
Metallic

2.  Intermolecular forces:

Solid Liquid Gas

Exit Slip

1.  Which of the following molecules exhibits covalent bonding?

a.  NaCl

b.  NH3

c.  CaO

d.  MgF2

2.  Ionic bonds DO NOT have the following characteristic

a.  Electrostatic attraction

b.  Cations and anions in a salt crystal

c.  Atoms that have exchanged electrons

d.  Atoms that have shared electrons

3.  Chlorine gas is a diatomic molecule. It is held together by:

a.  Ionic bonds

b.  Covalent bonds

c.  Metallic bonds

d.  Magnetic bonds

4.  When cations and anions join, they form this type of bond:

a.  Ionic

b.  Covalent

c.  Hydrogen

d.  Metallic

5.  Glucose (C6H12O6), glycine (NH2CH2COOH), and stearic acid (CH3(CH2)16COOH) are all molecules found in the human body. They bonds they form are:

a.  Nuclear

b.  Metallic

c.  Ionic

d.  Covalent

6.  The reason salt crystals, such as KCl, hold together so well is because the cations are strongly attracted to:

a.  Neighboring cations

b.  The protons in the nucleus of the neighboring atom

c.  Free electrons in the crystal

d.  Neighboring anions

7.  Which of the following molecules would be capable of conducting electricity in its solid form?

a.  MgCl2

b.  An Iron-nickel alloy

c.  Oxygen gas

d.  Hydrogen gas

8.  Which of the following statements is true about the melting points of ionic and covalent bonds?

a.  Ionic bonds have low melting points, while covalent bonds have slightly higher melting points

b.  Ionic bonds melt at very high temperatures, while covalent bonds have lower melting points

c.  Ionic and covalent bonds both have extremely high melting points.

d.  Ionic and covalent bonds both have low melting points.

9.  Which of the following is NOT a true of covalently bound molecules?

a.  Includes most biological molecules

b.  Able to conduct electricity in the form of a salt crystal

c.  Usually composed of two non-metals

d.  Have low melting points

10.  The following picture shows water in the ______phase of matter.

a.  Solid b. Liquid

c. Gas d. None of the above

11.  Under the same conditions of pressure and temperature, a liquid differs from a gas because the molecules of the liquid:

a.  Have no regular arrangement

b.  Are in constant motion

c.  Have stronger forces of attraction between them

d.  Take the shape of the container they are in

12.  Water and chlorine gas are both covalently bound compounds that exist at different states of matter. The reason they have different states of matter is due to:

a.  Ionic bonds

b.  Covalent bonds

c.  Intermolecular forces

d.  Hydrogen bonds

13.  In order for a compound to freeze from the liquid state into the solid state, attraction between particles must:

a.  Increase

b.  Decrease

c.  Remain the same

d.  Increase then decrease

Name: Date: Period:

Chemistry

Quiz #3: Ionic, Covalent, Metallic Bonding

  1. Which of the following molecules exhibits ionic bonding?
  1. NH3
  2. H2O
  3. H2
  4. MgCl2
  1. Glucose (C6H12O6) is an essential biological molecule. It is held together by:
  1. Ionic bonds
  2. Covalent bonds
  3. Metallic bonds
  4. Magnetic bonds
  1. Electrostatic attraction in a crystal lattice characterizes this type of bond:
  1. Ionic
  2. Covalent
  3. Metallic
  4. Magnetic
  1. The reason salt crystals, such as NaCl are held together so tightly is because the anions are strongly attracted to:
  1. Neighboring cations
  2. The protons in the nucleus of the neighboring atom
  3. Free electrons in the crystal
  4. Neighboring anions
  1. Which of the following molecules would be capable of conducting electricity when dissolved in solution?
  1. BeO
  2. Cl2
  3. CO2
  4. CH3Cl
  1. Choose the molecule with a low melting point that is often present in organic compounds.
  1. MgI2
  2. CO2
  3. BeO
  4. LiF
  1. This compound contains a free “sea” of electrons capable of conducting electricity in the solid form.
  1. Chlorine gas
  2. A salt composed of Sodium (Na) and Fluorine (F)
  3. An alloy of iron and copper
  4. Glucose (C6H12O6)
  1. In order for a compound to melt from the solid to the liquid state, the intermolecular attraction between particles must:
  1. Increase
  2. Decrease
  3. Remain the same
  4. Increase then decrease
  1. Solids differ from liquid because:
  1. The intermolecular bonds between particles in a solid are stronger than those in a liquid.
  2. The intermolecular bonds between particles in a liquid are stronger than those in a solid.
  3. Liquids particles are in constant, random motion while the particles in solids are not.
  4. Solid particles are in constant, random motion while the particles in liquid are not.
  1. What type of bond do all the molecules in the table above have in common?
  1. Covalent
  2. Ionic
  3. Metallic
  4. Polar