Chemistry Exam 1

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131 terms · 1406, Chapters 1-3, Timberlake

In this list, which substance can be classified as a chemical?

a. salt b. sleep c. cold d. heat e. temperature

Salt

Which of the following is not a chemical?

a. salt b. water c. light d. carbon dioxide e. sugar

Light

Chlorofluorocarbons are broken down in the atmosphere by ________.

a. nitrogen dioxide b. ozone c. iron d. AIDS e. ultraviolet light

UV Light

The production of smog from NO gas requires ________.

a. nitrogen b. chlorine c. water d. oxygen e. CFCs

Oxygen

Titanium dioxide is a chemical used in toothpaste to ________.

a. make the paste white b. disinfect the toothbrush c. keep the paste from spoiling d. remove plaque e. strengthen tooth enamel

Make paste White

21 cm is the same distance as

a. 0.0521 m. b. 52.1 dm. c. 5.21 mm. d. 0.00521 km. e. 5210 m.

0.0521 m.

How many centimeters are there in 57.0 in.?

a. 22 cm b. 0.0445 cm c. 145 cm d. 22.4 cm e. 140 cm

145 cm

The amount of space occupied by a substance is its...

a. mass. b. density. c. weight. d. length. e. volume.

Volume

Which of the following is a measurement of mass in the metric system?

a. milliliter b. centimeter c. kilogram d. Celsius e. meter

kilogram

A value of 36 mL is a measure of

a. density b. mass c. temperature d. volume e. distance

volume

The measurement 0.000 004 3 m, expressed correctly using scientific notation, is

4.3 x 10-7 m. b. 4.3 x 10-6 m. c. 4.3 x 106 m. d. 0.43 x 10-5 m. e. 4.3 m.

4.3 x 10-6 m.

Which of the following conversion factors is a measured number?

a. 10 cm/dm b. 12 in/ft c. 16 oz/lb d. 25 miles/gallon e. 12 eggs/dozen

25 miles/gallon

The measurement of the gravitational pull on an object is its

a. volume. b. weight. c. mass. d. length. e. size.

weight

1.00 pint of milk has a volume of how many milliliters? (2 pints = 1 quart)

a. 472 mL b. 530. mL c. 1000 mL d. 1890 mL e. 106 mL

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

The number of significant figures in the measurement of 45.030 mm is

a. none. b. three. c. four. d. five. e. six.

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

A calculator answer of 423.6059 must be rounded off to three significant figures. What answer is reported?

a. 423 b. 424 c. 1.7420 d. 423.6 e. 423.7

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

What is the correct answer for the calculation of a volume (in mL) with measured numbers ?

a. 0.22 mL b. 0.223 mL c. 57 mL d. 14 mL e. 14.3 mL

0.22 mL

The correct answer for the addition of 7.5 g + 2.26 g + 1.311 g + 2 g is
13.071 g. b. 13 g. c. 13.0 g. d. 10 g. e. 13.1 g.

13g

Which of the following measurements are not equivalent?
a. 25 mg = 0.025 g b. 183 L = 0.183 kL c. 150 ms = 0.150 s d. 84 cm = 8.4 mm e. 24 dL = 2.4 L

84 cm = 8.4 mm

Which of the following is the largest unit?
a. millimeter b. micrometer c. meter d. decimeter e. kilometer

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

Which of the following is the smallest unit?
a. gram b. milligram c. kilogram d. decigram e. microgram

microgram

9.31 g is the same mass as
931 μg. b. 931 kg. c. 93.1 cg. d. 9310 mg. e. 0.0931 dg.

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

How many pounds are in 3.5 kg?
a. 7.7 lb b. 1.59 lb c. 0.629 lb d. 1.6 lb e. 7.70 lb

7.7 lb

What is 6.5 m converted to inches?
a. 1700 in b. 1651 in c. 39 in d. 260 in e. 255.9 in

260 in

A nugget of gold with a mass of 521 g is added to 50.0 mL of water. The water level rises to a volume of 77.0 mL. What is the density of the gold?
a. 10.4 g/mL b. 6.77 g/mL c. 1.00 g/mL d. 0.0518 g/mL e. 19.3 g/mL

19.3 mL

A doctor's order is 0.125 g of ampicillin. The liquid suspension on hand contains 250 mg/5.0 mL. How many milliliters of the suspension are required?
a. 0.0025 mL b. 3.0 mL c. 2.5 mL d. 6.3 mL e. 0.0063 mL

2.5 mL

What is the mass of 2.00 L of an intravenous glucose solution with a density of 1.15 g/mL?
a. 0.0230 kg b. 2.30 kg c. 1.15 kg d. 0.0150 kg e. 0.575 kg

2.30 kg

What is the density of a substance with a mass of 45.00 g and a volume of 26.4 mL?
a. 1.70 g/mL b. 1.7 g/mL c. 0.59 g/mL d. 0.587 g/mL e. 45.0 g/mL

2.70 g/mL

A liquid has a volume of 34.6 mL and a mass of 46.0 g. What is the density of the liquid?
a. 1.00 g/mL b. 1.33 g/mL c. 0.752 g/mL d. 1330 g/mL e. 0.663 g/mL

1.33 g/mL

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?
a. 4.3 cm3 b. 4.29 cm3 c. 0.233 cm3 d. 53 cm3 e. 53.2 cm3

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.

A 50.0 mL urine sample has a mass of 50.7 g. The specific gravity of the urine is

a. 1.014 g/mL. b. 0.986 g/L. c. 1.01. d. 0.986. e. 50.7.

1.01

Coins in a piggy bank are an example of a(n)

a. compound. b. heterogeneous mixture. c. element. d. homogeneous mixture. e. none of the above

heterogeneous

Gold in a ring is a(n)

a. compound. b. heterogeneous mixture. c. element. d. homogeneous mixture. e. none of the above

element

Which of the following is a homogeneous mixture?

a. noodle soup b. water c. sugar d. tea e. carbon

tea

Which of the following is a heterogeneous mixture?

a. noodle soup b. water c. sugar d. tea e. carbon

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

Which of the following is a chemical change?

a. cutting a rope b. bending a steel rod c. making a snowman d. burning sugar e. melting gold

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

An example of kinetic energy is

a coiled spring. b. running water. c. a tree. d. natural gas. e. chemical energy.

running water

The energy associated with the motion of particles in a substance is called

a. temperature. b. electrical energy. c. heat. d. chemical energy. e. potential energy.

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

The phrase "ability to do work" is a definition of

a. specific heat. b. energy. c. calorie. d. heating. e. cooling.

energy

The energy stored in chemical bonds is

a. specific heat. b. kinetic energy. c. potential energy. d. work. e. a calorie.

potential energy

The energy of motion is referred to as
work. b. freezing. c. specific heat. d. potential energy. e. kinetic energy.

kinetic energy

In which of the following would the particles move most rapidly?

a. ice at -20 °C b. water at 20 °C c. steam at 110 °C d. boiling water e. ice at 0 °C

steam at 110

650. J is the same amount of energy as ________.

a. 155 cal b. 2720 cal c. 650. cal d. 1550 cal e. 2.72 cal

155 cal

3.25 kcal is the same amount of energy as ________.

a. 3.25 J b. 0.777 J c. 777 J d. 13600 J e. 13.6 J

13600 J

One cup of kidney beans contains 15 g of protein, 1 g of fat, and 42 g of carbohydrate. How many kilocalories, to two significant figures, does this sample contain? (The caloric values are: 4 kcal/g for carbohydrate, 9 kcal/g for fat, and 4 kcal/g for protein.)

a. 60. kcal b. 88 kcal c. 230 kcal d. 240 kcal e. 520 kcal

240 kcal

A cheeseburger from a fast food restaurant contains 19 g of fat, 20 g of carbohydrate, and 28 g of protein. How many kcal of energy does the cheeseburger contain? (The caloric values are: 4 kcal/g for carbohydrate, 9 kcal/g for fat, and 4 kcal/g for protein.) Give the answer to 2 significant figures.

a. 70. kcal b. 360 kcal c. 17 kcal d. 630 kcal e. 280 kcal

360 kcal

The dietary calorie(Cal) is equal to

a. 1000 kilocalories. b. 1000 calories. c. 100 calories. d. 10 calories. e. 1 calorie.

1000 calories

A temperature of 41 °F is the same as

a. 5 °C. b. 310 °C. c. -9 °C. d. 16 °C. e. 42 °C.

5 °C

If the temperature is 20. °C, what is the corresponding temperature on the Fahrenheit scale?

a. -22 °F b. 68 °F c. 43 °F d. 239 °F e. 94 °F

68 °F

A patient has a temperature of 38.5 °C. What is the temperature in degrees Fahrenheit?

a. 70.5 °F b. 311 °F c. 126.9 °F d. 101.3 °F e. 11.7 °F

101.3 °F

The temperature of liquid nitrogen is -196 °C. What is the corresponding reading on the Kelvin scale?

a. 77 K b. -127 K c. -91 K d. 48 K e. 146 K

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.

How many calories are required to raise the temperature of a 150. g sample of gold from 25 °C to 175 °C? The specific heat of gold is 0.0308 cal/g °C.

a. 4.62 cal b. 116 cal c. 22500 cal d. 693 cal e. 130. cal

693 cal

How many calories are required to increase the temperature of 13 g of alcohol from 11 °C to 23 °C? The specific heat of alcohol is 0.59 cal/g °C.

a. 83 cal b. 0.63 cal c. 92 cal d. 0.54 cal e. 170 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

The number of calories needed to raise the temperature of 32 g of water from 12 °C to 54 °C is
380 cal. b. 1.3 cal. c. 1300 cal. d. 1700 cal. e. 0.76 cal.

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

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?

a. 3.6 cal b. 3.6 x 103 cal c. 1.8 cal d. 80. cal e. 0.56 cal

3.6 x 103 cal

The formation of a gas resulting from the escape of high-energy particles from the surface of a liquid is known as

a. evaporation. b. deposition. c. boiling. d. melting. e. sublimation.

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.

The heat of fusion for water is 80. cal/g. How many calories of heat are released when 20.0 g of water at 0 °C is frozen to ice?

a. 620 cal b. 1600 cal c. 2000 cal d. 2200 cal e. 0 cal

1600 cal

The heat of fusion for water is 80. cal/g. How many calories of heat are needed to melt a 35 g ice cube that has a temperature of 0 °C?

a. 2300 cal b. 1600 cal c. 2800 cal d. 540 cal e. 0 cal

2800 cal

If the heat of vaporization for water is 540 cal/g, how many kilocalories are released when 5.00 g of steam is converted to liquid at 100 °C?

a. 540 kcal b. 5.0 kcal c. 110 kcal d. 2.7 kcal e. 5.4 kcal

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.

The sybol for aluminum is:
a. Al b. Am c. Au d. Sn e. Ag

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

Which of the following elements is a metal?

a. nitrogen b. fluorine c. argon d. strontium e. phosphorus

strontium

Which of the following elements is a nonmetal?

a. nitrogen b. sodium c. iron d. silver e. calcium

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

Which of the following elements is a noble gas?

a. oxygen b. chlorine c. bromine d. argon e. nitrogen

Argon

The smallest particle of an element that retains the characteristics of the element is a(n)

a. electron. b. neutron. c. proton. d. atom. e. nucleus.

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

What is the mass number of an atom of potassium that has 20 neutrons?

a. 15 b. 19 c. 35 d. 39 e. 59

39

Consider a neutral atom with 30 protons and 34 neutrons. The atomic number of the element is

a. 30. b. 32. c. 34. d. 64. e. 94.

30

Consider a neutral atom with 30 protons and 34 neutrons. The mass number for this atom is

a. 30. b. 32. c. 34. d. 64. e. 94.

64

____ 100. How many protons are in an isotope of sodium with a mass number of 25?

a. 11 b. 14 c. 15 d. 25 e. 32

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.

The correct symbol for the isotope of potassium with 22 neutrons is

a. 41/19K
b. 19/41K
c. 37/15K
d. 15/37K
e. 22/19K

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

The maximum number of electrons that may occupy the third electron energy level is

a. 2. b. 8. c. 10. d. 18. e. 32.

18

What is the element with the electron arrangement 2,8,7?

a. Be b. Cl c. F d. S e. Ar

Cl

What is the electron arrangement for aluminum?

a. 2,8,3 b. 2,8,5 c. 2,8,7 d. 2,8,8 e. 2,8,10

2, 8, 3

What is the electron arrangement for potassium (atomic number 19)?

a. 2,8,9 b. 2,8,7,2 c. 2,10,7 d. 2,8,8,1 e. 2,8,6,3

2, 8, 8, 1

What element has the electron arrangement 2,8,4?

a. carbon b. oxygen c. sulfur d. iron e. silicon

silicon

The number of electrons in the outer energy level of a neutral atom of boron (atomic number 5) is

a. 2. b. 3. c. 5. d. 8. e. 10.

3

Which element would have physical and chemical properties similar to chlorine?

a. Ar b. Br c. S d. O e. P

Br

What is the correct electron arrangement for the lithium atom?

a. 3 b. 3,1 c. 1,2 d. 2,1 e. 2,5

2, 1

The number of electron energy levels in a magnesium atom is

a. 1. b. 2. c. 3. d. 4. e. 5.

3

The element in this list with chemical properties similar to magnesium is

a. sodium. b. boron. c. carbon. d. strontium. e. chlorine.

stronium

Identify the noble gas in the following list.

a. helium b. nitrogen c. oxygen d. gold e. chlorine

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

Identify the metalloid in the following list.

a. sulfur b. fluorine c. silver d. copper e. germanium

germanium

The number of valence electrons found in an atom of a Group A element is equal to

a. its atomic number. b. its mass number. c. its group number. d. eight. e. eight minus the group number.

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

How many valence electrons are in the electron-dot symbols for the elements in group 3A(13)?

a. 1 b. 2 c. 3 d. 4 e. 6

3

The number of dots in the electron dot symbol of nitrogen is

a. one. b. two. c. three. d. four. e. five.

five

The number of dots in the electron dot symbol of carbon is

a. one. b. two. c. three. d. four. e. 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

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