Chem Test

14.Maximum number of electrons that can occupy the third principal energy level is a. 18 b. 32 c. 2 d. 8

A

17.According to Hund's rule: when electrons occupy orbitals of equal energy: one electron enters each orbit until a. All the orbitals contain one electron: with spins parallel b. All the orbitals contain one electron: with opposite spins c. There are two electrons in each orbital d. Electron velocities become constant

A

32.A metallic bond is a bond between a. Valence electrons and positively charged metal ions b. The ions of two different metals c. Metal and nonmetal d. None of the above

A

33.Which element when combined with chlorine would most likely form an ionic compound? a. Lithium b. Carbon c. Phosphorus d. Bromine

A

34.A cation is any atom or group of atoms with a. A positive charge b. No charge c. Negative charge d. More electrons than the corresponding atoms.

A

38.A diatomic molecule with a triple covalent bond is a. N2 b. Br2 c. H2 d. O2

A

49.Which of the following is an anion? a. O2- b. Mg2+ c. Al3+ d. H

A

71.Describe a sigma bond and pi bond.

A sigma bond is the end to end overlap of 2 s orbitals, an s orbital and p orbital, or 2 p orbitals. A pi bond is the side to side overlap of 2 p orbitals.

a. 1s2 2s2 2p6 3s2 3p1

Al

Name b. (NH4)2CO3

Ammonium carbonate

Name c. As2O5

Arsenic(V) oxide

11.The fourth principal energy level has a. 4 orbitals b. 16 orbitals c. 32 orbitals d. 9 orbitals

B

19.What is the maximum number of electrons that can occupy one orbital? a. 1 b. 2 c. 8 d. 18

B

20.The electron configuration for fluorine is a. 1s2 2s2 2p3 b. 1s2 2s2 2p5 c. 1s2 2s2 2p6 d. 1s2 2s2 2p6 3s2

B

22.The configuration for the outermost energy level in Ca is a. 3s2 b. 4s2 c. 2s1 d. 4s1

B

27.The electron configuration of fluoride ion; F- ; is a. 1s2 2s2 2p5 b. The same as that of the neon atom c. 1s2 2s2 2p6 3s1 d. The same as that of a potassium ion

B

29.In forming chemical bonds; atoms tend to attain a. State of higher energy b. Electron configuration of noble gas atoms c. Electron configuration of halogen atoms d. All of the above

B

31.Which of these is NOT a characteristic of most ionic compounds? a. Solid at room temperature b. Has a low melting point c. Conducts an electric current when melted d. Produced by reaction between metallic and nonmetallic elements

B

36.Which one of the following compounds is NOT covalent? a. SCl2 b. KCl c. HCl d. S2Cl2

B

41.Which of these compounds would NOT have covalent bonds? a. NO2 b. K2O c. N2O4 d. H2O2

B

42.A molecule with a single covalent bond is a. CO2 b. F2 c. NO d. N2

B

47.What is the formula for sulfuric acid? a. H2S2 b. H2SO4 c. H2SO3 d. H2S

B

51.What is the formula for aluminum oxide? a. AlO3 b. Al2O3 c. Al3O2 d. Al2O

B

12.If the electron configuration of an element is 1s2 2s2 2p6 3s2 3p5 the element is a. Iron b. Bromine c. Chlorine d. Phosphorus

C

18.What is the total number of orbitals in the third principal energy level? a. 1 b. 4 c. 9 d. 16

C

21.The atom whose electron configuration is 1s2 2s2 2p6 3s2 3p1 is a. B b. Na c. Al d. Ga

C

24.How many valence electrons does an atom of any element in Group 6A have? a. 2 b. 4 c. 6 d. 8

C

26.When an aluminum atom loses its valence electrons; what is the charge on the resulting ion? a. 2+ b. 2- c. 3+ d. 1+

C

28.Metals are good conductors of electricity because they a. Form crystal lattices b. Contain positive ions c. Contain mobile valence electrons D. Form Ionic bonds

C

35.The cation Fe3+ is formed when a. An atom of iron loses two electrons b. An atom of zinc loses two electrons c. An atom of iron loses three electrons d. An atom of iron gains three electrons

C

43.Correct name for the N3- ion is the: a. Nitrate ion b. Nitric ion c. Nitride ion d. Nitrite ion

C

44.Elements of group 14 a. Generally form positive ions b. Generally form negative ions c. Do not commonly form ions d. Do not combine with other elements

C

46.In naming a binary molecular compound; the number of atoms of each element present in the molecule is indicated by: a. Roman numerals b. Superscripts c. Prefixes d. Suffixes

C

48.Which of the following is a nonmetal? a. Iron b. Silver c. Oxygen d. Copper

C

53.The compound H3PO4 is named: a. Nitric acid b. Sulfuric acid c. Phosphoric acid d. Ethanoic acid

C

Name a. CS2

Carbon disulfide

Name d. CO

Carbon monoxide

c. 1s2 2s2 2p6 3s2 3p6 3d7 4s2

Co

Name a. CuCl

Copper(I) Chloride

13.The electron configuration of calcium is a. 1s2 2s2 2p2 3s2 3p3 4s2 b. 1s2 2s2 2p10 3s2 3p4 c. 1s2 2s2 3s2 3p6 3d8 d. 1s2 2s2 2p6 3s2 3p6 4s2

D

15.In order to occupy the same orbital two electrons must have a. The same direction of spin b. Low energy c. Opposite charge d. Opposite spin

D

16.Stable electron configurations are likely to contain a. High energy electrons b. Unfilled s orbitals c. Fewer electrons than unstable configurations d. Filled energy sublevels.

D

23.Among the following groups of atoms: which have the same outer energy level configurations? a. H: He b. Li; Be; N;Ne c. Mg; Al; Ca; Ga d. N; P; As; Bi

D

30.An ionic compound is a. Electrically neutral b. Held together by ionic bonds c. Composed of anions and cations d. All of the above

D

37.How many valence electrons does an atom of any halogen have? a. 1 b. 2 c. 4 d. 7

D

45.The metals in groups 1; 2; and 14; a. Gain electrons when they form ions b. Form ions with a charge found by subtracting 8 from the group number c. All form ions with a 1+ charge d. Lose electrons when they form ions

D

50.Among the following; which atom is most likely to form an ion with a charge of 2+ a. P b. Ma c. Al d. Ca

D

Name b. N2O3

Dinitrogen trioxide

a. KF what type of bond (F = 4.0 K = 0.8)

Ionic

b. 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6

Kr

74.In our most modern and accurate model, electrons in an atom are arranged in concentric (circular) orbits around the nucleus. AT/ST/NT

Never True

75.As many as 8 electrons may occupy the same orbital. AT/ST/NT

Never True

Name g. PI5

Phosphorus pentaiodide

b. SO2 what type of bond ( S= 2.5 O = 3.5)

Polar Covalent

c. NO2 what type of bond (N = 3.0 O = 3.5)

Polar Covalent

d. HBr what type of bond ( H= 2.1 Br = 2.8)

Polar Covalent

Name c. KC2H3O2

Potassium acetate

Name h. KMnO4

Potassium permanganate

Name f. H2SO4

Sulfuric acid

Name e. Sn(OH)4

Tin(IV) hydroxide