Chemistry Benchmark 1 Review: Question Preview (ID: 890)

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Which of the following Group 15 elements has the most metallic properties
a) Bi b) N c) Sb d) P
Pure silicon is chemically classified as a semi-metal because silicon
a) is malleable and ductile b) exhibits metallic and nonmetallic properties c) exhibits hydrogen bonding d) an excellent conductor of heat and electricity
The observed regularities in the properties of elements are periodic functions of their
a) atomic numbers b) nonvalence electrons c) oxidation states d) mass numbers
Elements in the Periodic Table are arranged according to their
a) atomic number b) relative size c) relative activity d) atomic mass
In which set do the elements exhibit the most similar chemical properties
a) N, O, and F b) Al, Si, and P c) Li, Na, and K d) H, Br, and Rn
Within Period 2 of the Periodic Table, as the atomic number increases, the atomic radius generally
a) decreases b) none of the above c) remains the same d) increases
Which of the following elements has the strongest attraction for electrons
a) boron b) sulfur c) oxygen d) aluminum
Atoms of which element has the weakest attraction for electrons
a) Na b) S c) Si d) P
As the elements in Group 2 are considered in order of increasing atomic number, the atomic radius of each element increases. This increase is due to an increase in
a) occupied electron orbitals b) ionic bonds between the valence electrons c) neutrons in the nucleus d) electrons in the outermost shell
Electronegativity is a measure of an atom's ability to
a) attract the electrons in the bond between one atom and another b) repel the protons of another atom c) attract the protons of another atom d) repel the electrons in the bond between one atom and another
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