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
Magnesium (Neutral )
Ve- =___
__
e- = __
P+ =__
Ve- =___
__
e- = __
P+ =__
12
3
Phosphorus (Neutral)
New Ion
Symbol
Lewis
Structure
e- = __
P+ =__
12
Magnesium
What must be done to make this
atom stable?
12
Ve- =___
__
New Ion
Symbol
Lewis
Structure
3
Phosphorus
e- = __
Ve- =___
__
P+ =__
What must be done to make this
atom stable?
12
3
3
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+
Identify each as either ionic or covalent compounds and provide either the name or formula
You may find these prefixes
helpful for the questions below
mono-
di-
tri-
tetra-
penta
hexa-
hepta
octa-
nona-
deca-
1
2
3
4
5
6
7
8
9
10
Ionic or
Covalent
11) dinitrogen trioxide
12) MgF2
13) phosphorus trifluoride
14) sulfur dioxide
15) N2O5
16) calcium nitrate
17) CO
18) lead (IV) oxide
19) FeSO4
20) H2O
Name or Formula
8 pts = ½ ea
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) _____________- Compounds have relatively weak force of attraction between molecules
26) _____________- Bonding occurs between nonmetals and nonmetals
27) _____________- When dissolved in water, it will conduct electricity
28) _____________- Bonding occurs when there is a sharing of valence electrons
Match each item with the correct statement below. NOTE: Each item may be used once, more than once, or not at all.
a.
b.
c.
d.
e.
f.
cation
anion
polyatomic ion
ionic compound
molecular compound
binary compound
g. electron configuration
h. electrostatic force
I. octet rule
j. valence electrons
k. electron dot structure
(Lewis Structure)
m. ionic bond
n. metallic bond
o. single covalent bond
p. double covalent bond
R. 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 ionicly 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. a covalent bond in which only one pair of electrons is shared
____ 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. compound composed of two different elements (can be ionic or molecular)
____ 45. this type of bond is found in table salt (NaCl)
____ 46. a covalent bond in which two pairs of electrons are shared
____ 47. phosphate PO43- is an example of a(n) _________
____ 48. the electrostatic force of attraction binding oppositely charged ions together
____ 49) What is the ionic charge on the Vanadium ion in the ionic compound Vanadium Sulfide, VS
?
____ 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 on the cation in FeCO3?
____ 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) Which of these elements does not exist as a diatomic molecule?
a. H
b. F
c. Ar
d. O
____ 60) Which of the following correctly provides the correct name and formula for each acid?
a. Sulfuric Acid – HSO4
c. Hydrochloric acid – H2Cl
b. Acetic Acid – HC2H3O2
d. Hydrophosphoric acid – H3PO4
____ 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.
____ 62) Under what conditions can potassium chloride conduct electricity?
a. only when melted
c. only when it is in crystal form
b. only when dissolved
d. only when melted or dissolved in water
____ 63) What is the basis of a metallic bond?
a. the attraction of metal cations to mobile electrons
b. the attraction between neutral metal atoms
c. the neutralization of protons by electrons
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
____ 66) Which of the following is not one of the seven diatomic elements?
a. O
b. Cl
c.He2
d. N
____ 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 binary 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
____ 76) What type of compound is PbSO ?
a. binary ionic b. polyatomic covalent
c. polyatomic ionic
d. binary molecular
____ 77) Which of the following is a binary molecular compound?
a. CaHSO
b. NaCl
c. He
d. CH4
____ 78) Which of the following formulas represents a molecular compound?
a. Ar
b. CO32c. 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. N O
d. PCl
____ 82) Which of the following compounds contains the lead(II) ion?
a. PbO
b. PbCl4
c. Pb2O
d. Pb2S
____ 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. K1d. 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) What is the charge/formula of the ion formed when tin achieves a stable electron configuration?
a. Sn2+
b. Sn1+
c. Sn1d. Sn2____ 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) 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.
____ 93) 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, SnF
2
____ 94) 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
95) What are the seven diatomic elements?
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
Cl2 ____________
N2 ____________
C2H4 ___________
Third exam = Chemical Bonding (4 pages) = 75 points + 3 EC = 104% possible (NOTE: This test will be applied toward your midterm)
Midterm = (Atomic Structure (2 pgs) + Matter & Measurements (2 pgs) = 4 pages = 90 points + 3 EC = 103% possible
OPTION: For you midterm, you can average in the third test (33%) + (66% from the midterm test)
Other than this third test on chemical bonding, you need to review your first two tests and practice tests
Matter & Measurements (Test 1)
-Accuracy, Precision, Calculating Density
-Percent Error (T# 10) (PT# 16)
-Determining Significant Figures (T# 12) (PT# 18)
-Unit Conversions (T# 13) (PT# 19)
-ROUNDING - Multiplication & Addition with Sig Figs (T# 14) (PT# 23)
-Making measurements (T# 15-16) (PT# 20-21)
-Scientific Notation (T# 17) (PT# 22)
-Classifying Matter (T# 21) (PT# 24)
-Properties vs. Changes (T# 22-37) (PT# 31-48)
-History of the atom (T# 38-45) (PT# 51-60)
-Multiple Choice & Short Answer & Other….
Atomic Structure (Test 2)
-Drawing Lewis Structures (T#4)
-Bohr Model of the atom (T# 5)
-Electron Configuration (T# 6)
-Periodic Table (T# 7)
-Periodic Trends: Atomic Radius, Ionization Energy, Electronegativity (T# 8-10)
-Terms (T# 20-31)
-Multiple Choice & Short Answer & Other….
All Three practice tests and answer keys are posted on my website: pearsongreatpath.wikispaces.com