PRACTICE TEST – Chemical Bonding (3rd Test) Name: ______

75 points + 3 EC = 104% possible

1-2) Complete the following problems for Magnesium and Phosphorus 5 points

Complete the table for both Monatomic & Polyatomic Ions below: 6 points = ½ point each

Name / Ion / Charge / / Name / Ion / Charge
3) sulfite / 7) / NH4 +
4) sulfide / 8) / O2-
5) hydroxide / 9) / CO3 2-
6) phosphide / 10) / Cu2+

Provide either the name or formula 6 points = 1/2 ea

Formula / Ions / Name
11) K2S
12) / Calcium Nitride
13) Mg3(PO4)2
14) / Amonnium carbonate
15) Ni(OH)2
16) / Cobalt (III) nitrite

17) Identify each of the following as being an Ionic compound, a Covalent molecule 6 points = 1/2 ea

Name / Ionic Covalent / Formula / Ionic Covalent
Iron (II) Oxide / Cl2
Dicarbon hexahydride / CaSO3
Potassium hydroxide / CoCO3
Nitrogen trihydride / H2O2

Identify each characteristic as being part of an IONIC Bond or a COVALENT Bond: 6 points

21) ______- Typically solids at room temperature

22) ______- Usually have high melting and boiling points

23) ______-Bonding occurs when there is a transfer valence electrons

24) ______- Bonding occurs between nonmetals and metals

25) ______- Bonding occurs when there is a sharing of valence electrons

26) ______- Bonding occurs between nonmetals and nonmetals

27) ______- Compounds contain positive and negative ions

28) ______- Compounds exist as neutral molecules

Match each item with the correct statement below. NOTE: Each item may be used once, more than once, or not at all.

A. cation G. electron configuration M. ionic bond

B. anion H. electrostatic force N. metallic bond

C. polyatomic ion I. octet rule O. covalent bond

D. ionic compound J. valence electrons P. solute

E. molecular compound K. electron dot structure R. solvent

F. solubility (Lewis Structure) S. crystal lattice

____ 29. the force of attraction between a positive and negative charge

____ 30. the element oxygen will gain two electrons to form a(n) ______

____ 31. the arrangement of electrons around the nucleus of an atom in its ground state

____ 32. atom or group of atoms having a positive charge

____ 33. a repeating pattern of cations and anions bonded together

____ 34. tightly-bound group of atoms that behaves as a unit and carries a net charge

____ 35. type of compound that forms a crystal lattice

____ 36. when one substance can “dissolve” in another substance this is known as ______

____ 37. type of compound composed only of non-metals that are covalently bonded together

____ 38. atoms react so as to acquire the stable electron structure of a noble gas with a full valence shell

____ 39. this type of bond is found in a molecule of water (H2O)

____ 40. a depiction (drawing) of valence electrons around the symbol of an element

____ 41. the electrons in the highest occupied energy level of an atom (outer most energy level)

____ 42. atom or group of atoms having a negative charge

____ 43. the electrostatic attraction between a sea of freely flowing valence electrons and metal cations

____ 44. when baking soda is added to vinegar, the baking soda dissolves and is considered a ______

____ 45. this type of bond is found in table salt (NaCl)

____ 46. when two atoms share valence electrons in order to become stable, this forms a ______

____ 47. phosphate PO43- is an example of a(n) ______

____ 48. the electrostatic force of attraction binding oppositely charged ions together

____ 49) An atom of aluminum will lose ____ electrons in order to obtain a noble gas electron configuration

____ 50) How many total covalent bonds will a nitrogen atom form in order to become stable?

____ 51) How many electrons does carbon need to share in order to obtain a noble-gas electron configuration?

____ 52) What is the charge of each of the oxygen atoms in covalent molecule O2?

____ 53) What is the net charge of the ionic compound sodium oxide?

____ 54) Which of the following elements does NOT form an ion with a charge of 2+ ?

a. magnesium b. calcium c. oxygen d. copper (II)

____ 55) Which of the following particles are free to drift in metals?

a. protons b. electrons c. neutrons d. cations

____ 56) Which of the following pairs of elements is most likely to form an ionic compound?

a. chlorine and oxygen c. aluminum and chlorine

b. nitrogen and sulfur d. sodium and lithium

____ 57) Which of the following is true about the melting temperature of dihydrogen monoxide?

a. The melting temperature is relatively high. c. The melting temperature is relatively low.

b. The melting temperature is variable and unpredictable. d. Dihydrogen monoxide does not melt.

____ 58) What characteristic of metals makes them good electrical conductors?

a. They have mobile valence electrons. c. They have mobile cations.

b. They have mobile protons. d. Their crystal structures can be rearranged easily.

____ 59) During the Hydrogen gas Lab H2 was created by splitting molecules of water, this was an example of

a. atoms forming a crystal lattice c. a physical change

b. atoms forming an ionic compound d. a chemical change

____ 61) How do atoms achieve noble-gas electron configurations (stability) in double covalent bonds?

a. Two atoms share one electron. c. Two atoms share two pairs of electrons.

b. Two atoms share two electrons. d. One atom completely loses two electrons to the other atom.

____ 63) What is the basis of a metallic bond?

a. the attraction of metal cations to mobile electrons c. the neutralization of protons by electrons

b. the attraction between neutral metal atoms d. the attraction of oppositely charged ions

____ 64) Which noble gas has the same electron configuration as the oxygen atom in a water molecule?

a. helium b. neon c. argon d. xenon

____ 65) Why do atoms share electrons in covalent bonds?

a. to become ions and attract each other c. by gaining or losing electrons to become stable

b. to attain a stable noble-gas electron configuration d. to increase their atomic numbers

____ 67) What type of ions have names ending in -ide?

a. only monatomic cations b. only monatomic anions c. only metal ions

____ 68) When Group 6A elements form ions, they ____.

a. lose two protons b. gain two protons c. lose two electrons d. gain two electrons

____ 69) When naming a transition metal ion that can have more than one common ionic charge, the numerical value of the charge is indicated by a ____.

a. prefix c. roman numeral following the name

b. suffix d. superscript after the name

____ 70) How are chemical formulas of ionic compounds generally written?

a. subscripts first, then ions c. Roman numeral first, then anion, then cation

b. cation on left, anion on right d. anion on left, cation on right

____ 71) Which of the following is NOT an anion?

a. hydroxide b. sulfate c. ClO1- d. iron(III) ion

____ 72) Which of the following is true about the composition of ionic compounds?

a. They are composed of cations and anions. c. They are composed of cations only.

b. They are composed of anions only. d. They are formed from two or more nonmetallic elements.

____ 73) Which element, when combined with bromine, would most likely form an ionic compound?

a. lithium b. carbon c. phosphorus d. chlorine

____ 74) What type of compound is CaO?

a. binary ionic b. polyatomic covalent c. polyatomic ionic d. binary molecular

____ 75) Which type of bond has the strongest electrostatic force of attraction between the atoms?

a)  Metallic b. ionic c. covalent d. all three have the same amount of electrostatic force

____ 77) Which of the following is true about the melting temperature of potassium chloride?

a. The melting temperature is relatively high. c. The melting temperature is relatively low.

b. The melting temperature is variable and unpredictable. d. Potassium chloride does not melt.

____ 78) Which of the following formulas represents a molecular compound?

a. Ar b. CO32- c. CuOH d. NO

____ 79) What does an -ite or -ate ending in a polyatomic ion mean?

a. Bromine is in the formula. c. Nitrogen is in the formula.

b. Sulfur is in the formula. d. Oxygen is in the formula.

____ 80) A repeating patterns of positive and negative ions held together by electrostatic attraction is a(n)

a. polyatomic ion b. crystal lattice c. diatomic molecule d. single covalent bond

____ 81) Which of the following formulas represents an ionic compound?

a. CS b. BaI c. NO d. PCl

____ 83) The octet rule states that, in chemical compounds, atoms tend to have ____.

a. the electron configuration of a noble gas c. more protons than electrons

b. eight electrons in their first (principal) energy level d. more electrons than protons

____ 84) What is the charge of the ion formed when potassium achieves noble-gas electron configuration?

a. K4+ b. K+ c. K1- d. K2-

____ 85) Which of the following elements does NOT form an ion with a charge of 1+ ?

a. fluorine b. hydrogen c. potassium d. sodium

____ 86) How can you determine if a compound is an acid?

a. there is an oxygen atom in the formula b. the first element is a hydrogen atom

b. the net charge will be zero d. it will have both a metal and a non-metal

____ 87) Which of the following occurs in an ionic bond?

a. Oppositely charged ions attract. c. Two atoms share more than two electrons.

b. Two atoms share two electrons. d. Like-charged ions attract.

____ 88) What is the net charge of the ionic compound calcium fluoride?

a. 2– b. 1– c. 0 d. 1

____ 89) What is the name of the ionic compound formed from lithium and bromine?

a. lithium bromine b. lithium bromide c. lithium bromium d. lithium bromate

____ 90) Which of the following compounds has the formula KNO?

a. potassium nitrate b. potassium nitride c. potassium nitrite d. potassium nitrogen oxide

____ 91) Which of the following pairs of elements is most likely to form an ionic compound?

a. magnesium and fluorine c. oxygen and chlorine

b. nitrogen and sulfur d. sodium and aluminum

____ 92) In which of the following is the name and formula given correctly?

a. sodium oxide, NaO c. cobalt (II) chloride, CoCl

b. barium nitride, BaN d. tin(II) fluoride, SnF2

93) What does an atom react?

96) Explain why Mono-atomic atoms do not bond. Provide an example of a mono-atomic atom. 3 points

97) Compare and Contrast Ionic and covalent bonds. 3 points

a) how are they similar?

b) how are they different?

98) Complete the Lewis Structures for each Compound 4 points

99) What is a precipitate?

100) During the “Hydrogen Gas Lab” what was some observable evidence that a chemical reaction was occurring?

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