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Chemistry
Mid Term Exam Review
Name ___________________________
1) Read the temperature with the correct number of significant figures.
A) 87°C
B) 87.2°C
C) 87.20°C
D) 87.200°C
E) 87.2000°C
2) Which of the following statements is TRUE?
A) A scientific law is fact.
B) Once a theory is constructed, it is considered fact.
C) A hypothesis is speculation that is difficult to test.
D) An observation explains why nature does something.
E) A scientific law summarizes a series of related observations
3) Which of the following statements about the phases of matter is TRUE?
A) In both solids and liquids, the atoms or molecules pack closely to one another.
B) Solids are highly compressible.
C) Gaseous substances have long-range repeating order.
D) There is only one type of geometric arrangement that the atoms or molecules in any solid can
adopt.
E) Liquids have a large portion of empty volume between molecules.
4) Choose the heterogeneous mixture from the list below.
A) sports drink
B) chlorine gas
C) black coffee
D) chicken noodle soup
E) carbon (graphite)
5) All of the following are SI base units of measurement, EXCEPT
A) meter
B) gram
C) second
D) kelvin
E) mole
6) Which of the following are examples of intensive properties?
A) density
B) volume
C) mass
D) None of the above are examples of intensive properties.
E) All of the above are examples of intensive properties.
7) Determine the density of an object that has a mass of 149.8 g and displaces 12 .1 mL of water
when placed in a graduated cylinder.
A) 8.08 g/mL
B) 1.38 g/mL
C) 12 .4 g/mL
D) 18.1 g/mL
E) 11.4 g/mL
8) Systematic error is defined as
A) error that tends to be too high or too low.
B) error that has equal probability of being too high and too low.
C) error that averages out with repeated trials.
D) error that is random.
E) None of the above.
9) What answer should be reported, with the correct number of significant figures, for the
following calculation? (433.621 - 333.9) × 11.900
A) 1.19 × 103
B) 1.187 × 103
C) 1.1868 × 103
D) 1.18680 × 103
E) 1.186799 × 103
10) If an object has a density of 8.65 g/cm3, what is its density in units of kg/m3?
A) 8.65 × 10-3 kg/m3
B) 8.65 × 10-7 kg/m3
C) 8.65 × 103 kg/m3
D) 8.65 × 101 kg/m3
E) None of the above
11) Which of the following is an example of the law of multiple proportions?
A) A sample of chlorine is found to contain three times as much Cl-35 as Cl-37.
B) Two different compounds formed from carbon and oxygen have the following mass ratios:
1.33 g O: 1 g C and 2.66 g O: 1 g C.
C) Two different samples of table salt are found to have the same ratio of sodium to chlorine.
D) The atomic mass of bromine is found to be 79.90 amu.
E) Nitrogen dioxide always has a mass ratio of 2.28 g O: 1 g N.
12) Determine the number of protons, neutrons and electrons in the following:
40
18 X
A) p+ = 18 n° = 18
B) p+ = 18 n° = 22
C) p+ = 22 n° = 18
D) p+ = 18 n° = 22
E) p+ = 40 n° = 22
e- = 22
e- = 18
e- = 18
e- = 40
e- = 18
13) Which of the following statements about subatomic particles is TRUE?
A) A neutral atom contains the same number of protons and electrons.
B) Protons have about the same mass as electrons.
C) Electrons make up most of the mass of an atom.
D) Protons and neutrons have opposite, but equal in magnitude, charges.
E) Neutrons and electrons are found in the nucleus of an atom.
14) Give the number of electrons in P-3.
A) 18
B) 12
C) 19
D) 15
E) 16
15) Which of the following elements is a metalloid?
A) Al
B) Ge
C) C
D) Sn
E) Pb
16) Gallium has an atomic mass of 69.723 amu. The Ga-69 (68.926 amu) is 60.11%. What is the
amu of the other isotope?
A) 70.924 amu
B) 70.928 amu
C) 70.932 amu
D) 70.920 amu
E) 69.723 amu
17) How many moles are in 2.16 x 1024 atoms of lead?
A) 35.9 moles
B) 3.59 moles
C) 0.359 moles
D) 6.08 moles
E) 1.79 moles
18) Who determined the charge of an electron?
A) Millikan
B) Thomson
C) Chadwick
D) Rutherford
E) Einstein
19) Which of the following does NOT describe a nonmetal?
A) tend to gain electrons
B) found in the upper right hand corner of the periodic table
C) poor conductor of electricity
D) nonmetals are generally unreactive
E) poor conductor of heat
20) An ionic bond is best described as
A) the sharing of electrons.
B) the transfer of electrons from one atom to another.
C) the attraction that holds the atoms together in a polyatomic ion.
D) the attraction between 2 nonmetal atoms.
E) the attraction between 2 metal atoms.
21) Which of the following is a molecular compound?
A) CuCl2
B) KCl
C) NaNO3
D) CH3Cl
E) RbBr
22) Which of the following is an ionic compound?
A) SCl2
B) Mg3(PO4)2
C) Cl2O
D) CH2O
E) PF5
23) Write the formula for the compound formed between potassium and sulfur.
A) KS
B) KS2
C) K2S
D) K2SO3
E) K3S2
24) Calculate the molar mass of Ca3(PO4)2.
A) 87.05 g/mol
B) 215.21 g/mol
C) 310.18 g/mol
D) 279.21 g/mol
E) 246.18 g/mol
25) What is the mass of 9.44 × 1024 molecules of NO2? The molar mass of NO2 is 46.01 g/mol.
A) 205 g
B) 294 g
C) 721 g
D) 341 g
E) 685 g
26) How many sodium ions are contained in 99.6 mg of Na2SO3? The molar mass of Na2SO3 is
126.05 g/mol.
A) 1.52 × 1027 sodium ions
B) 4.76 × 1020 sodium ions
C) 2.10 × 1021 sodium ions
D) 1.05 × 1021 sodium ions
E) 9.52 × 1020 sodium ions
27) Determine the empirical formula for a compound that contains C, H and O. It contains
52.14% C and 34.73% O by mass.
A) C2H6O
B) CHO
C) C4H13O2
D) CH4O3
E) CH3O
28) Which of the following has the smallest mass?
A) 3.50 × 1023 molecules of I2
B) 85.0 g of Cl2
C) 2.50 mol of F2
D) 0. 050 kg of Br2
E) All have the same mass
29) Write a balanced equation to show the reaction of sulfurous acid with lithium hydroxide to
form water and lithium sulfite.
A) H2SO4 (aq) + LiOH (aq) → H2O (l) + Li2SO4 (aq)
B) H2SO3 (aq) + 2 LiOH (aq) → 2 H2O (l) + Li2SO3 (aq)
C) HSO3 (aq) + LiOH (aq) → H2O (l) + LiSO3 (aq)
D) HSO4 (aq) + LiOH (aq) → H2O (l) + LiSO4 (aq)
E) H2S (aq) + 2 LiOH (aq) → 2 H2O (l) + Li2S (aq)
30) How many moles of NaCl are required to make 250 mL of a 3.00 M solution?
A) 750 moles
B) 0.750 moles
C) 3 moles
D) 0.250 moles
E) None of the above.