# Chemistry Exam 1

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1406, Chapters 1-3, Timberlake

Salt

Light

UV Light

Oxygen

Make paste White

0.0521 m.

145 cm

Volume

kilogram

volume

4.3 x 10-6 m.

25 miles/gallon

weight

472 mL

### Which of the following numbers contains the designated correct number of significant figures? a. 0.04300 5 significant figures b. 0.00302 2 significant figures c. 156 000 3 significant figures d. 1.04 2 significant figures e. 3.0650 4 significant figures

156 000 - 3 SigFigs

five

### Which of the following examples illustrates a number that is correctly rounded to three significant figures? a. 4.05438 grams to 4.054 grams b. 0.03954 grams to 0.040 grams c. 103.692 grams to 103.7 grams d. 109 526 grams to 109 500 grams e. 20.0332 grams to 20.0 grams

20.0332 grams to 20.0 grams

424

### Which of the answers for the following conversions contains the correct number of significant figures? a. 2.543 m x 39.4 in/1m = 100.1942 in b. 2 L x 1.06qt/1L = 2.12 qt c. 24.95 min x 1hr/60min = 0.4158 hr d. 12.0 ft x 12in/1ft x 2.54cm/1in = 370 cm e. 24.0 kg x 1lb/2.20kg = 11 lb

24.95 min x 1hr/60min = 0.4158 hr

0.22 mL

13g

84 cm = 8.4 mm

kilometer

### What is the metric relationship between grams and micrograms? a. 1 g = 100 μg b. 1 g = 1 000 000 μg c. 1 g = 0.000 001 μg d. 1 g = 1000 μg e. 1 g = 0.001 μg

1 g = 1 000 000 μg

microgram

9310 mg

### Which of the following setups would convert centimeters to feet? a. cm x 2.54/1cm x 1ft/12in b. cm x 2.54cm/1in x 12in/1ft c. cm x 1in/2.54cm x 1ft/12in d. cm x 1in/2.54cm x 12in/1ft e. cm x 2.54cm/1in x 1ft/12in

cm x 1in/2.54cm x 1ft/12in

7.7 lb

260 in

19.3 mL

2.5 mL

2.30 kg

2.70 g/mL

1.33 g/mL

4.29 cm3

### The EPA limit for lead in the soil of play areas is 400 ppm. This is the same as a. 400 mg lead in each gram of soil. b. 400 g lead in each kilogram of soil. c. 400 mg lead in each kilogram of soil. d. 400 µg lead in each kilogram of soil. e. 400 µg lead in each milligram of soil.

400 mg lead in each gram of soil.

1.01

heterogeneous

element

tea

noodle soup

### Which of the following is an example of a physical change? a. grinding coffee beans b. baking a cake c. converting water to hydrogen and oxygen d. digesting a cheeseburger e. burning coal

grinding coffee beans

### Which of the following would not be a physical change? a. freezing water to make ice cubes b. tearing a piece of aluminum foil c. boiling water for soup d. burning gasoline in a lawnmower e. melting gold to make jewelry

burning gasoline in a lawnmower

burning sugar

### Which of the following is a chemical change? a. burning natural gas b. melting ice c. hammering gold into foil d. cutting a tomato e. cutting paper

burning natural gas

running water

heat

### Which of the following is an example of potential energy? a. chewing food b. water stored in a reservoir c. burning wood d. a fan blade turning e. riding an exercise bike

water stored in a reservoir

energy

potential energy

kinetic energy

steam at 110

155 cal

13600 J

240 kcal

360 kcal

1000 calories

5 °C

68 °F

101.3 °F

77 K

### Absolute zero is a. the freezing point of water using the Celsius scale. b. the boiling point of liquid nitrogen. c. the temperature on the Kelvin scale corresponding to 32 °F. d. the coldest temperature possible. e. the freezing point of liquid nitrogen.

the coldest temperature possible.

### A kilocalorie of heat is required to raise the temperature of a. 1 g of water from 14 °C to 15 °C. b. 1 g of water by 10 °C. c. 10 g of water by 10 °C. d. 100 g of water by 10 °C. e. 100 g of water by 100 °C.

100 g of water by 10 °C.

693 cal

92 cal

### The specific heat of copper is 0.092 cal/g °C, and the specific heat of silver is 0.057 cal/g °C. If 100 cal of heat is added to one g of each metal at 25 °C, what is the expected result? a. The copper will reach a higher temperature. b. The silver will reach a higher temperature. c. The two samples will reach the same temperature. d. The copper will reach a temperature lower than 25 °C. e. The silver will soften.

The silver will reach a higher temperature

### Which of the following quantities is not required to calculate the amount of heat energy required to heat water from 25 °C to 55 °C? a. the mass of the water sample b. the initial temperature c. the final temperature d. the specific heat of water e. the heat of vaporization for water

the heat of vaporization for water

### Raising the temperature of 10.0 g of water from 10.0 °C to 20.0 °C requires 100.0 cal of energy, while raising the temperature of 10.0 g of aluminum from 10.0 °C to 20.0 °C requires 22.0 cal. More calories are required to heat the water because a.water is a liquid and aluminum is a solid at 10.0 °C. b. ten grams of water occupies a larger volume than 10.0 g of aluminum. c. water has a greater potential energy than aluminum. d. water has a larger specific heat than aluminum. e. 10.0 °C is closer to the melting point of water than to the melting point of aluminum.

water has a larger specific heat than aluminum

1300 cal

### Which of the following is a property of a solid? a. It takes the shape of the container. b. It fills the volume of the container. c. The particles move at a rapid rate. d. The interactions between its particles are very weak. e. The particles have fixed positions and are very close together.

The particles have fixed positions and are very close together.

### In a gas, the distance between the particles is a. very close relative to the size of the molecules. b. close relative to the size of the molecules. c. fixed relative to the size of the molecules. d. small relative to the size of the molecules. e. very large relative to the size of the molecules.

very large relative to the size of the molecules

### Which one of the following properties describes a liquid? a. has its own shape b. particles are close together and move randomly c. particles move very rapidly d. fills the entire volume of the container e. There is essentially no interaction between the particles.

particles are close together and move randomly

3.6 x 103 cal

evaporation

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

the steam will give off a large amount of heat as it condenses.

1600 cal

2800 cal

2.7kcal

### Which of the following does not involve a change of state? a. melting ice b. freezing water c. vaporization of alcohol d. sublimation of dry ice e. pouring water into a vacuum-insulated bottle

pouring water into a vacuum-insulated bottle

### A heating curve illustrates a. what a substance looks like as it is heated. b. what happens to the particles of a substance as it is heated. c. what happens to the heat applied as the temperature is increased. d. the changes in the temperature and physical state of a substance as it is heated. e. the chemical changes that occur as the substance is heated.

the changes in the temperature and physical state of a substance as it is heated.

### On a heating curve a plateau corresponds to a. a change in temperature of a liquid. b. a change in temperature of a solid. c. a change in temperature of a gas. d. a change of state. e. the solid being broken into smaller pieces.

a change in temperature of a solid

### Which of the following does not represent a step on the heating curve of water? a. The temperature of steam cannot exceed 100 °C. b. The temperature of ice remains at 0 °C as it melts. c. The temperature of liquid water increases linearly as it is heated. d. The temperature of liquid water remains at 100 °C as it boils. e. Both liquid water and ice are present at 0 °C.

The temperature of steam cannot exceed 100 °C.

Al

### What elements are in hydroxyapatite, Ca5(PO4)3OH, a major compound in human bones and teeth? a. carbon, potassium, oxygen, hydrogen b. calcium, phosphorous, oxygen, hydrogen c. carbon, phosphorous, oxygen, helium d. calcium, phosphorous, oxygen, helium e. carbon, potassium, oxygen, helium

calcium, phosphorous, oxygen, hydrogen

### Which of the following properties is not a characteristic of the Group 1A(1) elements (alkali metals)? a. They are shiny. b. They are good conductors of heat. c. They react vigorously with water. d. Most of them are liquids at room temperature. e. They are good conductors of electricity.

Most of them are liquids at room temperature.

### The Group 8A(18) elements a. are unreactive and are rarely found in combination with other elements. b. are good conductors of electricity. c. melt at high temperatures. d. are liquids at room temperature. e. react vigorously with water.

are unreactive and are rarely found in combination with other elements

strontium

nitrogen

### Which of the following is a characteristic of nonmetals? a. shiny b. malleable c. good conductors of heat d. low melting points e. good conductors of electricity

low melting points

Argon

atom

### According to the atomic theory, a. all atoms are different. b. atoms are neither created nor destroyed during a chemical reaction. c. atoms of the same element combine to form compounds. d. all matter is made up of tiny particles called electrons. e. a compound can contain different numbers of atoms as long as it has the same kinds of atoms.

atoms are neither created nor destroyed during a chemical reaction

### Which of the following descriptions of a subatomic particle is correct? a. A proton has a positive charge and a mass of approximately 1 amu. b. An electron has a negative charge and a mass of approximately 1 amu. c. A neutron has no charge and its mass is negligible. d. A proton has a positive charge and a negligible mass. e. A neutron has a positive charge and a mass of approximately 1 amu.

A proton has a positive charge and a mass of approximately 1 amu.

### In an atom, the nucleus contains a. an equal number of protons and electrons. b. all the protons and neutrons. c. all the protons and electrons. d. only neutrons. e. only protons.

all the protons and neutrons.

### The number of neutrons in an atom is equal to a. the atomic number. b. the mass number. c. the mass number + the atomic number. d. the mass number - the atomic number. e. the number of protons.

the mass number - the atomic number

### The mass number of an atom can be calculated from a. the number of electrons. b. the number of protons plus neutrons. c. the number of protons. d. the number of electrons plus protons. e. the number of neutrons.

the number of protons plus neutrons

39

30

64

11

### Which of the following gives the correct numbers of protons, neutrons, and electrons in a neutral atom of ? a. 118 protons, 50 neutrons, 118 electrons b. 118 protons, 118 neutrons, 50 electrons c. 50 protons, 68 neutrons, 50 electrons d. 68 protons, 68 neutrons, 50 electrons e. 50 protons, 50 neutrons, 50 electrons

50 protons, 68 neutrons, 50 electrons

### Isotopes are atoms of the same element that have a. different atomic numbers. b. the same atomic numbers but different numbers of protons. c. the same atomic numbers but different numbers of electrons. d. the same atomic number but different numbers of neutrons. e. the same atomic mass but different numbers of protons.

the same atomic number but different numbers of neutrons.

41/19K

### 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? a. The atomic mass of chlorine will be less than 35. b. The atomic mass of chlorine will be more than 37. c. You cannot tell what the atomic mass will be. d. The atomic mass will be between 35 and 37. e. The atomic mass will be 24.3.

The atomic mass will be between 35 and 37

### Which of the following is not true for the atoms 13N, 14N, and 15N? a. They all have the same mass number. b. They are isotopes. c. They all have the same atomic number. d. They all have 7 protons. e. They all have 7 electrons.

They all have the same mass number.

### The elements lithium, sodium, and potassium a. are isotopes of each other. b. are in the same period of elements. c. have the same number of neutrons. d. are in the same group. e. have the same mass number.

are in the same group

### The electron arrangement of any particular atom shows a. the number of isotopes possible. b. a description of the shape of each electron energy level. c. the number of electrons in each energy level. d. a diagram of an atomic nucleus. e. the maximum number of electrons each energy level can hold.

the number of electrons in each energy level

18

Cl

2, 8, 3

2, 8, 8, 1

silicon

3

Br

2, 1

3

stronium

helium

### Semiconductors are located in the periodic table on (or in) the a. left side of the table. b. right side of the table. c. line dividing metals from nonmetals in the table. d. first period of the table. e. last period of the table.

line dividing metals from nonmetals in the table

germanium

its group number

### Valence electrons are electrons located a. in the outermost energy level of an atom. b. in the nucleus of an atom. c. in the innermost energy level of an atom. d. throughout the atom. e. in the first three shells of an atom.

in the outermost energy level of an atom

### In an electron-dot symbol of an element, the dots are used to represent a. all of the electrons in the atom. b. the valence electrons. c. the electron arrangement. d. only the electrons that will participate in bond formation. e. the electrons that the element will gain when it forms a compound.

the valence electrons

3

five

four

### The atomic size of atoms a. increases going across a period. b. decreases going across a period. c. decreases going down within a group. d. does not change going across a period. e. none of the above

decreases going across a period

### The atomic size of atoms a. increases going across a period. b. decreases going down within a group. c. increases going down within a group. d. does not change going down within a group. e. none of the above

increases going down within a group

### The ionization energy of atoms a. decreases going across a period. b. decreases going down within a group. c. increases going down within a group. d. does not change going down within a group. e. none of the above

decreases going down within a group

### Ionization energy is a. the energy an ion acquires from an electron. b. the energy needed to remove the least tightly bound electron. c. highest for metals in Group 1A(1). d. higher for potassium than for lithium. e. none of the above

the energy needed to remove the least tightly bound electron

### The metallic character of elements a. increases going across a period. b. decreases going down within a group. c. increases going down within a group. d. does not change going down within a group. e. none of the above

increases going down within a group

Example: