AP Chemistry Semester 1 Test Questions

Silica that has been doped with Arsenic would be considered which type of semiconductor? A. N-type semiconductor B. P-type semiconductor C. Super-conductor D. Nonmetal conductor

A. N-type semiconductor

The oxygen-carbon-oxygen bond angle in CO2 is A. 120 B. 109.5 C. 180 D. 90 axial, 120 equatorial

C. 180

An atom of silicon in its ground state is subjected to a frequency of light that is high enough to cause electron ejection. An electron from which subshell of silicon would have the highest kinetic energy after ejection? A. 1s B. 2p C. 3p D. 4s

C. 3p

Which element will have a higher electronegativity value: chlorine or bromine? Why? A. Chlorine, because it has less electron shielding B. Bromine, because it has more protons C. Chlorine, because it is smaller D. Bromine, because it is larger

C. Chlorine, because it is smaller

Which of the following compounds does NOT have a TETRAHEDRAL structure? A. CH4 B. NH4+ C. SF4 D. AlCl4

C. SF4

The hybridization of carbon in CH4 is A. Sp B. Sp2 C. Sp3 D. Dsp

C. Sp3

What hybridization of the OXYGEN atoms CO2? A. both sp3 B. sp3, sp2 C. both sp2 D. sp2, sp E. both sp

C. both sp2

Which of the following atoms below is LEAST likely to violate the octet rule? A. Be B. P C. S D. B E. F

E. F

Identify the shape of XeF4

square planar

Identify the shape of H2CO

trigonal planar

Identify the shape of NF3

trigonal pyramidal

Which of the following BEST explains the strength of diamond over graphite? A. Carbon atoms in graphite are able to move past each other in the network B. Carbon atoms in Diamond form a tetrahedral shape with Sp3 hybridization which creates a stronger, hexagonal network than graphite which has a trigonal planar shape and Sp2 hybridization C. Graphite has London dispersion forces which are weaker than the strong Dipole-Dipole forces in diamond, giving diamond stronger covalent network D. The single sigma bonds in diamond are much stronger than the sigma and pi bonds present in graphite, giving diamond a stronger covalent network

?

Which of the following lists of species is in order of increasing boiling points? A. H2, N2, NH3 B. N2, NH3, H2 C. NH3, H2, N2 D. NH3, N2, H2

?

Why can a molecule with the structure of NBr5 not exist? A. Nitrogen only has two energy levels and is thus unable to expand its octet B. Bromine is much larger than nitrogen and cannot be a terminal atom in this molecule C. It is impossible to complete the octets for all six atoms using only valence electrons D. Nitrogen does not have a low enough electronegativity to be the central atom of this molecule

A. Nitrogen only has two energy levels and is thus unable to expand its octet

The wavelength range for infrared radiation is 10^-5 m, while that of ultraviolet radiation is 10^-8 m. Which type of radiation has more energy, and why? A. Ultraviolet has more energy because it has a higher frequency B. Ultraviolet has more energy because it has a longer wavelength C. Infrared has more energy because it has a lower frequency D. Infrared has more energy because it has a shorter wavelength

A. Ultraviolet has more energy because it has a higher frequency

What is the most likely electron configuration for a sodium ion in its ground state? A. 1s2, 2s2, 2p5 B. 1s2, 2s2, 2p6 C. 1s2, 2s2, 2p6, 3s1 D. 1s2, 2s2, 2p5, 3s2

B. 1s2, 2s2, 2p6

Which of the following pairs of elements is most likely to create an interstitial alloy? A. Titanium and Copper B. Aluminum and Lead C. Silver and Tin D. Magnesium and Calcium

B. Aluminum and Lead

A liquid whose molecules are held together by only which of the following forces would be expected to have the lowest boiling point? A. Ionic Bonds B. London Dispersion forces C. Hydrogen Bonds D. Metallic Bonds

B. London Dispersion forces

Which neutral atom of the following elements would have the most unpaired electrons? A. Titanium B. Manganese C. Nickel D. Zinc

B. Manganese

Which of the following compounds would have the highest lattice energy? A. LiF B. MgCl2 C. CaBr2 D. C2H6

B. MgCl2 (Charge)

Why does CaF2 have a higher melting point than NH3? A. CaF2 is more massive and thus has stronger London Dispersion Forces. B. CaF2 exhibits network covalent bonding, which is the strongest type of bonding. C. CaF2 is smaller and exhibits greater Coulombic attractive forces. D. CaF2 is an ionic substance and it requires a lot of energy to break up an ionic lattice.

D. CaF2 is an ionic substance and it requires a lot of energy to break up an ionic lattice.

Which of the following statements is true regarding sodium and chlorine? A. Sodium has a greater electronegativity and a larger first ionization energy B. Sodium has a larger first ionization energy and a larger atomic radius C. Chlorine has a larger atomic radius and a greater electronegativity D. Chlorine has a greater electronegativity and a larger first ionization energy

D. Chlorine has a greater electronegativity and a larger first ionization energy

Which of the following molecules would exhibit the strongest dipole moment? A. CH4 B. BCl3 C. PBr5 D. OF2

D. OF2

Why does an ion of phosphorus P3-, have a larger radius than a neutral atom of phosphorus? A. There is greater Coulombic attraction between the nucleus and the electrons in P3- B. The core electrons in P3- exert a weaker shielding force than those of a neutral atom C. The nuclear charge is weaker in P3- than it is in P D. The electrons in P3- have a greater electron-electron repulsion than those in the neutral atom

D. The electrons in P3- have a greater electron-electron repulsion than those in the neutral atom

Which of the following elements has its highest energy subshell completely full? A. Sodium B. Aluminum C. Chlorine D. Zinc

D. Zinc

Is CF4 polar or nonpolar?

Nonpolar

Is H2 polar or nonpolar?

Nonpolar

Is H2CO polar or nonpolar?

Polar

Is H2S polar or nonpolar?

Polar

Identify the shape of HCN

linear