Title: Final Exam-Fall 2015
Course: DOL Grant Introduction to Chemistry

Q: Write 0.000 000 33 in scientific notation.
- 3.3 × 10<sup>7</sup>
- 3.3 × 10<sup>-7</sup>
- 3.3 × 10<sup>-8</sup>
- 3.3 × 10<sup>8</sup>
- 3.3
A: 3.3 × 10<sup>-7</sup>

Q: In the number 123.45, the digit 5 is in the hundreds place.
- True
- False
A: False

Q: The correct answer for the addition of 7.5 g + 2.26 g + 1.311 g + 2 g is ________.
- 13.071 g
- 13 g
- 13.0 g
- 10 g
- 13.1 g
A: 13 g

Q: Diamond has a density of 3.52 g/mL. What is the volume in cubic centimeters of a diamond with a mass of 15.1 g?
- 4.3 cm<sup>3</sup>
- 4.29 cm<sup>3</sup>
- 0.233 cm<sup>3</sup>
- 53 cm<sup>3</sup>
- 53.2 cm<sup>3</sup>
A: 4.29 cm<sup>3</sup>

Q: A dose of aspirin of 5.0 mg per kilogram of body weight has been prescribed to reduce the fever of an infant weighing 8.5 pounds. The number of milligrams of aspirin that should be administered is ________.
- 19 mg
- 53 mg
- 1.6 mg
- 5.0 mg
- 0.59 mg
A: 19 mg

Q: The number 650 000 has two significant figures.
- True
- False
A: True

Q: When the measured number 0.0090 is multiplied by the measured number 87.10, the answer has two significant figures.
- True
- False
A: True

Q: A patient has a temperature of 38.5 °C. What is the temperature in degrees Fahrenheit?
- 70.5 °F
- 311 °F
- 126.9 °F
- 101.3 °F
- 11.7 °F
A: 101.3 °F

Q: A potato contains 20 g of carbohydrate. If carbohydrate has a caloric value of 4 kcal/g, how many kcal are obtained from the carbohydrate in the potato?
- 5 kcal
- 20 kcal
- 40 kcal
- 60 kcal
- 80 kcal
A: 80 kcal

Q: If the heat of fusion for water is 80. cal/g, how many calories are needed to melt 45.0 g of ice at 0 °C?
- 3.6 cal
- 3.6 × 10<sup>3</sup> cal
- 1.8 cal
- 80. cal
- 0.56 cal
A: 3.6 × 10<sup>3</sup> cal

Q: A burn from steam at 100 °C is expected to be more severe than a burn from boiling water at 100 °C because ________.
- the steam is hotter than the boiling water
- there is more steam than water
- the steam will give off a large amount of heat as it condenses
- you are more likely to come into contact with the steam than with the boiling water
- All of these answers are correct.
A: the steam will give off a large amount of heat as it condenses

Q: A sample of chlorine has two naturally occurring isotopes. The isotope Cl-35 makes up 75.8% of the sample, and the isotope Cl-37 makes up 24.3% of the sample. Which of the following statements is true?
- The atomic mass of chlorine will be less than 35.
- The atomic mass of chlorine will be more than 37.
- You cannot tell what the atomic mass will be.
- The atomic mass will be between 35 and 37.
- The atomic mass will be 24.3.
A: The atomic mass will be between 35 and 37.

Q: Consider a neutral atom with 30 protons and 34 neutrons. The mass number for this atom is ________.
- 30
- 32
- 34
- 64
- 94
A: 64

Q: How many valence electrons are in the electron-dot symbols for the elements in group 3A (13)?
- 1
- 2
- 3
- 4
- 6
A: 3

Q: Identify the noble gas in the following list.
- helium
- nitrogen
- oxygen
- gold
- chlorine
A: helium

Q: The Group 8A (18) elements ________.
- are unreactive and are rarely found in combination with other elements
- are good conductors of electricity
- melt at high temperatures
- are liquids at room temperature
- react vigorously with water
A: are unreactive and are rarely found in combination with other elements

Q: Consider an isotope of sodium with a mass number of 25. The number of neutrons in this isotope of sodium is ________.
- 11
- 14
- 16
- 25
- 32
A: 14

Q: Ionization energy is ________.
- the energy an ion acquires from an electron
- the energy needed to remove the least tightly bound electron
- highest for metals in Group 1A (1)
- higher for potassium than for lithium
- None of these
A: the energy needed to remove the least tightly bound electron

Q: Metallic character increases going down a group.
- True
- False
A: True

Q: Atomic size decreases going from left to right within a period.
- True
- False
A: True

Q: The proton is 2000 times the mass of the neutron.
- True
- False
A: False

Q: A sodium atom with a mass number of 23 has 23 neutrons.
- True
- False
A: False

Q: A polar covalent bond is found in which of these compounds?
- H<sub>2</sub>O
- F<sub>2</sub>
- NaCl
- H<sub>2</sub>
- N<sub>2</sub>
A: H<sub>2</sub>O

Q: A group of covalently bonded atoms that has an overall electrical charge is called a(n) ________.
- ionic compound
- anion
- polyatomic ion
- cation
- molecule
A: polyatomic ion

Q: An anion always ________.
- has a positive charge
- contains a group of two or more atoms with a positive charge
- contains a metal and a nonmetal
- forms covalent bonds
- has a negative charge
A: has a negative charge

Q: Elements in group 2A (2) of the periodic table form ions with a charge of ________.
- 1+
- 1-
- 2+
- 3+
- 0
A: 2+

Q: In ionic compounds, ________ lose their valence electrons to form positively charged ________.
- metals, anions
- nonmetals, cations
- metals, polyatomic ions
- nonmetals, anions
- metals, cations
A: metals, cations

Q: How many electrons will aluminum gain or lose when it forms an ion?
- lose 1
- gain 5
- lose 2
- lose 3
- gain 1
A: lose 3

Q: The carbon tetrachloride molecule, CCl<sub>4</sub>, has the shape of a ________.
- tetrahedron
- square
- cube
- circle
- sphere
A: tetrahedron

Q: The number of electrons in an ion with 16 protons and an ionic charge of 2- is ________.
- 16
- 18
- 20
- 22
- 24
A: 18

Q: What is the symbol for the ion with 19 protons and 18 electrons?
- F<sup>+</sup>
- F<sup>-</sup>
- Ar<sup>+</sup>
- K<sup>-</sup>
- K<sup>+</sup>
A: K<sup>+</sup>

Q: The main type of attractive forces between molecules of ammonia (NH<sub>3</sub>) are ________.
- ionic bonds
- hydrogen bonds
- polar covalent
- dipole-dipole attractions
- dispersion forces
A: hydrogen bonds

Q: The main type of attractive forces between molecules of carbon tetrabromide (CBr<sub>4</sub>) are ________.
- ionic bonds
- hydrogen bonds
- polar covalent
- dipole-dipole attractions
- dispersion forces
A: dispersion forces

Q: The ability of an atom to attract the shared electrons in a covalent bond is its ________.
- electronegativity
- bonding ability
- polarity
- ionic character
- nonpolarity
A: electronegativity

Q: Which of the following is an oxidation-reduction reaction?
- CaCl<sub>2</sub> + Na<sub>2</sub>SO<sub>4</sub> <img align="middle" height="17" width="13" src="ppg/pearson/tm/ichem12t/u8594.gif"/> CaSO<sub>4</sub> + 2NaCl
- KOH + HNO<sub>3</sub> <img align="middle" height="17" width="13" src="ppg/pearson/tm/ichem12t/u8594.gif"/> H<sub>2</sub>O + KNO<sub>3</sub>
- N<sub>2</sub> + O<sub>2</sub> <img align="middle" height="17" width="13" src="ppg/pearson/tm/ichem12t/u8594.gif"/> 2NO
- AgNO<sub>3</sub> + NaCl <img align="middle" height="17" width="13" src="ppg/pearson/tm/ichem12t/u8594.gif"/> AgCl + NaNO<sub>3</sub>
- Al<sub>2</sub>(SO<sub>4</sub>) <sub>3</sub> + 6KOH <img align="middle" height="17" width="13" src="ppg/pearson/tm/ichem12t/u8594.gif"/> 2Al(OH)<sub>3</sub> + 3K<sub>2</sub>SO<sub>4</sub>
A: N<sub>2</sub> + O<sub>2</sub> <img align="middle" height="17" width="13" src="ppg/pearson/tm/ichem12t/u8594.gif"/> 2NO

Q: The molar mass of C<sub>3</sub>H<sub>8</sub>O<sub>2</sub> is ________.
- 76.09 g/mole
- 60.09 g/mole
- 29.02 g/mole
- 69.02 g/mole
- 52.01 g/mole
A: 76.09 g/mole

Q: In the following reaction, what is the correct coefficient for aluminum chloride?<br/><br/><img align="bottom" src="ppg/pearson/tm/ichem12t/f24g1q37g1.gif"/><br/>
- 1
- 2
- 3
- 4
- 5
A: 2

Q: In a ________ reaction, two or more elements or compounds form one product.
- decomposition
- single replacement
- combustion
- double replacement
- combination
A: combination

Q: 0.400 mole of sucrose, C<sub>12</sub>H<sub>22</sub>O<sub>11</sub>, contains ________ C atoms.
- 12
- 6.02 × 10<sup>23</sup>
- 5.02 × 10<sup>22</sup>
- 2.89 × 10<sup>24</sup>
- 4.80
A: 2.89 × 10<sup>24</sup>

Q: <i>For the following question(s), consider the following equation. <br/></i><br/><img align="bottom" src="ppg/pearson/tm/ichem12t/f24g1q51g1.gif"/><br/><br/><br/>The number of moles of oxygen gas needed to react with 4.0 moles of Mg is ________.
- 1.0 mole
- 2.0 moles
- 3.0 moles
- 4.0 moles
- 6.0 moles
A: 2.0 moles

Q: According to the kinetic theory of gases, a gas can be compressed much more than a liquid or solid because ________.
- a gas is composed of very small particles
- the particles of a gas are very far apart
- gas particles move rapidly
- gas particles do not attract or repel one another
- gas particles move faster when the temperature increases
A: the particles of a gas are very far apart

Q: A 5.00-L tank contains helium gas at 1.50 atm. What is the pressure of the gas in mmHg?
- 1.50 mmHg
- 507 mmHg
- 760 mmHg
- 1140 mmHg
- 3800 mmHg
A: 1140 mmHg

Q: A gas at 5.00 atm pressure was stored in a tank during the winter at 5.0 °C. During the summer, the temperature in the storage area reached 40.0 °C. What was the pressure in the gas tank in the summer?
- 0.625 atm
- 4.44 atm
- 5.63 atm
- 40.0 atm
- 69.5 atm
A: 5.63 atm

Q: In water, a substance that ionizes completely in solution is called a ________.
- weak electrolyte
- nonelectrolyte
- semiconductor
- nonconductor
- strong electrolyte
A: strong electrolyte