Unit 6 – Chemistry Flashcard

If the atoms that share electrons have polar bonds, then electrons…

A. are transferred
B. generally have a difference in electronegativities of less than .3
C. are equally shared between atoms
D. are not equally shared between atoms
E. form ionic bonds

D
Hydrogen bonding would be seen in a sample of which of the following substances?

A. CH4
B. H20
C. H2
D. all of the answer choices
E. CCL4

B
The pair of elements that forms a bond with the least ionic character is

A. Na and Cl
B. Br and Cl
C. Ga and Cl
D. I and I
E. H and Cl

D
The Ga-F bond in GaF3 is (electronegativity for Ga is 1.6; for F is 4.0) is

A. metallic
B. nonpolar covalent
C. pure covalent
D. polar covalent
E. ionic

E
In which of these compounds is the bond between the atoms a polar covalent bond?

A. I2
B. Br2
C. F2
D. S8
E. HF

E
In a molecule of oxygen gas, the four shared electrons give each oxygen atom __electrons in the outer energy level.

A. 8
B. 32
C. 4
D. 2
E. 18

A
Which of the following lists of species is in order of increasing boiling point?

A. H2, NH3, N2
B. NH3, H2, N2
C. H2, N2, NH3
D. NH3, N2, H2
E. N2, NH3, H2

C
Solid NaCl melts at a temperature of 800 degrees Celsius. Which of the following is an explanation for the higher melting point of NaCl?

A. a chlorine ion is larger than a bromine ion
B. a chlorine ion has a lesser negative charge than a bromine ion
C. a chlorine ion has less mass than a bromine ion
D. a chlorine ion is smaller than a bromine ion
E. a chlorine ion has a greater negative charge than a bromine ion

D
Which of the compounds listed below would require the greatest energy to separate it into ions in the gaseous state?

A. MgO
B. NaCl
C. Na2O
D. Nal
E. MgCl2

A
Which of the molecules listed below has the largest dipole moment?

A. HCl
B. SO3
C. Cl2
D. NO
E. N2

A
Otis, the cat, and Mollie, a canine chemistry friend, had a late night discussion about Group 16 elements. An element from Group 16 would most likely form an ionic bond with an element from

A. Group 15
B. Group 18
C. Group 2
D. Group 16
E. Group 17

C
The Lewis structure for the aluminum ion has

A. 3 valence electrons
B. 13 valence electrons
C. 0 valence electrons
D. 8 valence electrons
E. 5 valence electrons

D
Multiple covalent bonds may occur in atoms that contain oxygen, nitrogen, or

A. carbon
B. magnesium
C. hydrogen
D. chlorine
E. helium

A
A liquid whose molecules are held together by which of the following forces would be expected to have the lowest boiling point?

A. ionic bonds
B. London dispersion forces
C. metallic bonds
D. network bonds
E. hydrogen bonds

B
In metals, the valence electrons

A. are attached to particular positive ions
B. are not involved in the bonding
C. are in an electron sea
D. are immobile
E. form covalent bonds

C
Which best explains the observation that metals are malleable and ionic crystals are brittle?

A. van der Waals forces
B. their polarity
C. their chemical bonds
D. their London forces
E. their heats of vaporization

C
The person whose work led to a periodic table based on increasing atomic mass was

A. Seaborg
B. Mosely
C. Rutherford
D. Camnizzaro
E. Mendeleev

E
What is the correct formula for potassium phosphide?

A. KP
B. P2K
C. K3P
D. KP3
E. K3PO3

C
Name the compound CuCO3

A. cupric trioxycarbide
B. cuprous carbide
C. copper (II) carbonate
D. Copper (I) carbonate
E. copper cobalt

C

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