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CHEMISTRY I
MID-TERM ASSESSMENT
Indicate the letter of the best answer on your answer sheet.
Objective 1.01: Design, conduct and analyze investigations to answer questions related to
chemistry.
Objective 1.02: Evaluate reports of scientific investigations from an informed scientificallyliterate viewpoint.
Objective 1.03: Evaluate experimental designs with regard to safety.
1. Which of the following is quantitative data?
a. Color
c. Odor
b. Shape
d. Volume
2. Which procedure represents the safest technique to use for diluting a concentrated acid?
a. Add the acid to the water quickly
b. Add the acid slowly to the water with steady stirring
c. Add the water to the acid quickly.
d. Add the water slowly to the acid with steady stirring
Use the diagram below for question 3.
3. A biochemist is performing an experiment to determine the effects of Chemical X on the growth
of bacteria. Which tube is the experimental control?
a. Test tube 1
b. Test tube 2
c. Test tube 3
d. Test tube 4
Objective 2.01: Analyze the historical development of the current atomic theory.
4. Which sequence represents a correct order of historical developments leading to the modern model of
the atom?
a. The atom is a hard spheremost of the atom is empty space with a small dense
nucleuselectrons exist in orbitals outside the nucleus
b. The atom is a hard sphereelectrons exist in orbitals outside the nucleusmost of the atom is
empty space with a small dense nucleus.
c. Most of the atom is empty space with a small, dense nucleuselectrons exist in orbitals outside
the nucleusthe atom is a hard sphere.
d. Most of the atom is empty space with a small dense nucleusthe atom is a hard
sphereelectrons exist in orbitals outside the nucleus.
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5. According to the modern model of the atom, which of the following best shows the behavior of
electrons?
a.
b.
c.
d.
Orbiting the nucleus in fixed paths.
Found in regions outside the nucleus called orbitals.
Combined with neutrons in the nucleus.
Located in a solid sphere covering the nucleus.
6. The diagram below shows the results of Rutherford’s experiment in which he used a radioactive
source to “shoot” alpha particles at a thin sheet of gold foil. Based on these results, what were
Rutherford’s conclusions?
a. Atoms are solid matter with positive and negative charges scattered throughout.
b. Atoms are solid, positively charged matter with negatively charged electrons scattered
throughout.
c. Atoms are mostly empty space with small, dense, positively charged centers.
d. Atoms are mostly empty space with small, dense, negatively charged centers.
Objective 2.02: Examine the nature of atomic structure including subatomic particle, mass
number, atomic number and isotopes.
7. Compared to a proton, an electron has
a. A greater amount of charge and the same sign
b. A greater amount of charge and the opposite sign
c. The same amount of charge and the same sign
d. The same amount of charge and the opposite sign
8. Which pair of particles is found in the nucleus?
a. Proton and electron
b. Proton and neutron
c. Neutron and electron
d. Neutron and beta particle
9. Which symbols represent atoms that are isotopes?
a.
b.
c.
d.
C-14 and N-14
O-16 and O-18
I-131 and I-131
Rn-222 and Ra-222
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10. An ion with 8 protons, 8 neutrons, and 10 electrons is represented by
a. Ne
b. O+2
c. O-2
d. O
11. What is the mass number of an atom which contains 28 protons, 28 electrons, and 34 neutrons?
a.
b.
c.
d.
28
56
62
90
Use the chart below to answer question 12.
12. The chart shows isotopes of some common elements. In what two properties do the
isotopes of carbon differ?
a.
b.
c.
d.
Atomic number and number of neutrons
Atomic mass and number of neutrons
Atomic mass and number of protons
Number of protons and number of neutrons
Objective 2.03: Apply the language and symbols of chemistry.
You may need to use your reference tables to answer these questions.
13. What is the chemical formula for a compound formed from calcium ions (Ca2+) and chloride ions
(Cl–)?
a. CaCl
b. Ca2Cl
c. CaCl2
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d. Ca2Cl2
14. What is the correct formula for aluminum oxide?
A AlO
B Al3O2
C AlO2
D Al2O3
15. What is the Stock system name for FeO?
A Iron oxide
B Iron (II) oxide
C Iron (III) oxide
D Iron oxygen
16. What is the correct name for the compound NH4Cl?
A nitrogen chloride
B nitrogen chlorate
C ammonium chloride
D ammonium chlorate
17. What is the formula for nitrogen trifluoride?
A NiF3
B NF3
C N3F
D Ni3F
Objective 2.04: Identify substances using their physical properties.
You may need to use your reference tables to answer these questions.
Use the chart below on questions 18 and 19.
A student is determining the density of a U.S. nickel. His data is shown below:
# of
Mass
Mass
Mass
Volume
Volume
Volume
nickels
graduated
cylinder,
nickels
of water
of water
of nickels
cylinder
water,
and
and
and
nickels
50 ml
nickels
water
15
50.00g
73.50g
18. What is the mass of 15 nickels?
a. 73.50g
b. 29.00g
?
50.0 ml
53.0 ml
c. 79.00g
19. What is the average density of the nickels?
a. 7.8 g/ml
b. 8.9 g/ml
c. 8.2 g/ml
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?
d. 5.50g
d. 1.1 g/ml
Density of
nickels.
?
e. 23.50g
20. Given the diagrams X, Y, and Z below. Which diagram or diagrams represent a mixture of elements
A and B?
A
B
C
D
X only
Z only
X and Y
X and Z
21. A physical change occurs when
A a peach spoils
B a bracelet turns your wrist green
C a copper bowl tarnishes
D a glue gun melts a glue stick
22. What substance has a melting point of -94 C and a boiling point of 65 C?
a. Ethanol
b. Chlorine
c. Hexane
d. Methanol
23. 22.4 liters of a gas has a mass of 36.5 grams. What is the identity of the gas?
a. Chlorine
b. Hydrogen chloride
c. Nitrogen
d. Hydrogen
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Objective 2.06: Assess bonding in metals and ionic compounds as related to chemical and
physical properties.
24.
This apparatus was most likely designed to show that —
A the formation of an ionic compound is an exothermic reaction
B ionic compounds conduct a current in solution
C the formation of an ionic compound is an endothermic reaction
D water is a good conductor of electricity
Use the chart below on questions 25-27
25. What type of bonding is mostly likely in compound A?
a. ionic
b. non-polar covalent
c. polar covalent
d. metallic
26. What type of bonding is most likely in compound C?
a. ionic
b. non-polar covalent
c. polar covalent
d. metallic
27. What type of bonding is most likely in compound D?
a. ionic
b. non-polar covalent
c. polar covalent
d. metallic
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Use the diagram below in question 28.
28. The diagram represents the arrangement of atoms in a metallic solid. Scientists believe that
electrons in the outer energy levels of the bonding metallic atoms are free to move from one atom
to the next. Because they are free to move, these electrons are often referred to delocalized
electrons and give metals ALL of the following properties EXCEPT.
a. Conduct heat and electricity in the solid state.
b. Brittle, break easily
c. Malleable and ductile.
d. Luster
Objective 2.07: Assess covalent bonding in molecular compounds as related to chemical and
physical properties and molecular geometry.
29. Which of the following substances best illustrates polar covalent bonding?
a. HCl
b. NaBr
c. CsF
d. Cl2
30. The methane, CH4, gas molecule exhibits what type of geometric shape?
a. trigonal planar
b. tetrahedral
c. bent or V-shaped
d. trigonal pyramidal
31. Which substance would have London dispersion forces as the main type of intermolecular forces
of attraction?
a. H2O
b. F2
d. HCl
d. NaCl
32. Diamond, graphite, and silicon dioxide all exhibit which type of intermolecular force?
a. metallic
b. network covalent
c. ionic
d. hydrogen e. dipole-dipole
33. Which of the following compounds contains polar bonds, yet the molecule itself is nonpolar?
B.
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34. Which diagram best represents the structure of a water molecule?
C
35. Which of the following is the correct electron dot structure for N2?
Answer
Objective 3.01: Analyze periodic trends in chemical properties and use the periodic table to
predict properties of elements.
36 If two elements have similar chemical properties, which of the following would be similar in
both elements?
a. atomic radii
b. number of energy levels
c. number of valence electrons
d. atomic mass
37. Which of the following is the correct noble gas configuration for iron?
a. [Ar] 3d64s2
b. [Ne] 3d64s2
c. [Xe] 3d64s6
d. [Ca] 4s2
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Use the Chart Below to Answer Questions 38-42
1
18
2
A
B
13
3
4
5
6
7
8
9
10
11 12
14 15 16
C
38. Which element has the highest ionization energy?
a. A
b. B
c. C
d. D
e. E
39. Which element is most likely to gain electrons?
a. A
b. B
c. C
d. D
e. E
40. What is the electron configuration of element C?
a. 1s2, 2s2, 2p6
b. 1s2, 2s2, 2p1
c. 1s2, 2s2, 3s1
d. 2s2, 2p3
41. What element is a metalloid?
a. A
b. B
c. C
d. D
e. E
42. Which element has the largest atomic radii?
a. A
b. B
c. C
d. D
e. E
43. What is the orbital notation for a chlorine atom in the ground state.
C
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17
D
E
Objective 3.02: Apply the mole concept, Avogadro’s number and conversion factors to
chemical calculations.
44. 5.00 moles of sodium have a mass of
a. 4.60 g
c. 23.0 g
b. 115 g
d. 55.0 g
45. How many molecules of hydrogen chloride gas (HCl) are in 73.0g of the gas.
a. 6.02 x 1023 molecules
c
12.0 x 1023 molecules
b. 36.5 molecules
d
1.5 molecules
.
46. Which conversion factor would you use to calculate correctly the mass of 2 moles of the element
titanium?
a. 1 mol Ti
47.9 g Ti
c. 22.4 L Ti
1 mol Ti
b. 6.02 x 1023
1 mol Ti
d. 47.9 g Ti
1 mol Ti
47. Which compound has the smallest molar mass?
a a. CO
c H2O
.
b b. CO2
d H2O2
.
.
Objective 4.01: Analyze the Bohr model in terms of electron energies in the hydrogen atom.
Use the Reference Tables to answer questions 48-50.
48. Which type of electromagnetic energy has the shortest wave length?
a.
Visible light
b.
Radio waves
c.
Ultraviolet radiation
d.
Gamma radiation
49. The mathematical equation c= λf means that as the wavelength (λ) increases, the frequency (f)
decreases. The equation E = hf means that as frequency increases, energy increases. Using this
information and the reference tables, which color of visible light has the least energy?
a.
Red
b.
Yellow
c.
Green
d.
Violet
50. If an electron drops from n=6 to n=2, what type of electromagnetic radiation is emitted?
a.
Ultraviolet (UV)
b.
Visible
c.
Infrared (IR)
d.
Radiowaves
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