Test Ch 1

1.Identify the activity that belongs in the field of chemistry.

a. developing medicines c. production of a new plastic

b. analysis of a compound d. all of the above

2. Which of the following tasks would probably not be assigned to an analytical chemist?

a. Determine the amount of copper in a sample.

b. Determine the amount of lead in a blood sample.

c. Determine the least expensive method to produce nylon

d. Determine the amount of pollutants in a local lake.

3. Which of these chemicals is definitely inorganic?

a. one that is made of carbon and hydrogen

b. one that is made of nitrogen and carbon

c. one that is made of nitrogen and hydrogen

d. one that is made of carbon and oxygen

4. Identify the false statement.

a. Chemistry plays an important role in efforts to increase the world´s food supply and to

protect crops.

b. Biodiesel is a fossil fuel.

c. potatoe plants with a jellyfish gene will glow when they need to be watered.

d. chemists are working to develop more pest-resistant and disease-resistant plants.

5. A hypothesis is

a. an observation recorded from an experiment.

b. a proposed explanation for what is observed.

c. a summary of the results of many experiments.

d. a well-tested explanation for many observations.

6. Which of the following is not a part of the scientific method?

a. experimenting c. proving

b. observing d. hypothesizing

7. A well-tested explanation for a broad set of observations is

a. a hypothesis c. a theory

b. an experiment d. a scientific law.

8. To which of the following might a hypothesis be elevated after repeated experimentation?

a. observation c. theory

b. scientific law d. experiment

9. Define chemistry.

___________________________________________________________________________

___________________________________________________________________________

___________________________________________________________________________

___________________________________________________________________________

10.List the major steps in the scientific method.

__________________________________________________________________________

__________________________________________________________________________

__________________________________________________________________________

11. List the 5 traditional branches of chemistry.

_________________________________ ___________________________________

_________________________________ ___________________________________

_________________________________

Ch 2

Match the definition on column B to the term on column A. Write the correct letter on the line.

Column A Column B

_______ 1. Product a. matter that flows but has a definite volume

_______ 2. Phase b. amount of matter that an object contains

_______ 3. Physical change c. starting substance in a chemical reaction

_______ 4.liquid d. homogeneous mixture

_______ 5. Mass e. the simplest form of matter with a unique set of

properties

_______ 6. Element f. a part of a sample with uniform composition and

properties

______ 7. Solid g. alters a substance without changing its

composition

______ 8.solution h. matter with a definite shape and volume

______ 9. Compound i. substance formed in a chemical reaction

______ 10. Reactant j. contains two or more elements chemically

combined in a fixed proportion

True-False

AT always true ST sometimes true NT never true

______ 11. Any part of a sample with uniform composition and properties is called a phase.

______ 12. A substance does not have a fixed composition

______ 13. A heterogeneous mixture consists of two or more phases.

______ 14. A vapor is a gaseous substance that is generally a liquid at room temperature.

______ 15. A compound can be physically separated into its elements.

Multiple choice

______ 16. Another name for homogenous mixture is

a. Solution b. matter c. element d. mass

______ 17. The chemical symbol for iron is

a. Ir b.FE c. Fe d. I

______ 18. Which of the following is a physical property?

a. Color b. hardness c. freezing point d.all of the above

______ 19. Which of the following statements describes a solid?

a. It takes the shape of its containerb. It takes the volume of its containerc. Its particles are packed together tightly.d. It is easily compressed.

______ 20. At room temperature, which of the following is typically in a physical state different

from that of the other three.

a. Water b. milk c. grape juice d. oxygen

______ 21. Which of the following is an example of a physical change?

a. Toasting bread c. digesting a bananab. Cooking a hamburger d. melting butter

______ 22. An example of a heterogenous mixture would be

a. Sugar b.salt water c.tap water d. vegetable soup

______ 23. Which of the following is a compound?

a. Carbon b.hydrogen c.oxygen d. water

_____ 24. The element whose chemical symbol is C is

a. calcium b. carbon c. copper d. chlorine

______ 25.Which of the following events can best distinguish a physical change from a chemical

change?

a. Energy is absorbed or released c. a gas is producedb. A different chemical composition d. Mass is conserved

______ 26. Which of the following is an example of a chemical change?

a. Cooking meat c. dissolving sugar in iced teab. Slicing cheese d. freezing water

______ 27. Homogeneous mixtures

a. Are always liquids c. have a composition that is fixedb. Consists of two or more phases d. are known as solutions

______ 28. A compound

a. Is a pure substance c. can be physically separated into its elementsb. Has a composition that varies d. has properties similar to those of its elements

______ 29. Physical properties of a substance include

a. Color and odor c. malleabilityb. Melting and boiling points. d all of the above

______ 30. When iron and oxygen combine to form iron oxide,

a. A physical change occurs c. a change in mass occursb. A change of state occurs d. a chemical change occurs

Completion

31. A _____________________________ is a form of matter that flows, has a fixed volume, and takes the shape of its container.

32. A _____________________________ is a gaseous substance that is generally a liquid or solid at room temperature.

33. A tossed green salad is an example of a _________________________ mixture.

34. The chemical symbol for the element nitrogen is _____________________.

35. In a chemical reaction, the starting substances are called ________________________.

36. The burning of wood is an example of a _________________________ change.

37. The evaporation of water is an example of a _______________________ change.

38. Any matter that has a uniform and definite composition is a (n) _______________________.

Ch 3

Matching

Column A Column B

______ 1. Error a. a measure of the pull of gravity on a given mass

______ 2. Precision b. concerned with the reproducibility of measurements

______ 3. 1 liter c. a ratio of equivalent measurements

______ 4. Temperature d. originally defined as the mass of 1 L of water at 4° C

______ 5. Density e. a way to analyze and solve problems using the units of a measurement

______6. Conversion factor f. the ratio of the mass of an object to its volume

______7. Dimensional analysis g. the degree of hotness or coldness of an object

______ 8. Weight h. closeness of a measurement to the true value

______ 9. 1 kilogram i. difference between the experimental value and the accepted value.

______ 10. Accuracy j. the volume of a cube 10 cm on each edge

Multiple choice

______ 11. How many significant figures are in the measurement 2103.2 g ?

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

______ 12. Which of these equalities is not correct?

a. 100 cg= 1 g c. 1 cm3 = 1 mlb. 1000 mm= 1 m d. 10kg = 1 g

______ 13. How many of the zeros in the measurement 0.000040200 m are significant?

a. 2 c. 7b. 3 d. 8

______ 14. How many milligrams are in 2.5 kg?

a. 2.5 x 10 mg c. 2.5 x 10 mgb. 25 mg d. 2.5 x 10 mg

______ 15. The closeness of a measurement to its true value is a measure of its:

a. Usefulness c. accuracyb. Precision d. reproducibility

______ 16. Which of these measurements is expressed to three significant figures?

a. 0.070 m c. 7007 mgb. 7.30 x 10 d..007 m

______ 17. A metric unit of volume is the:

a. L c. kmb. Mg d. K

______ 18. The number of seconds in a 40- hour week can be calculated as follows:

a. C.

b. d.

______ 19. The metric prefix kilo means:

a.100 times smaller c. 1000 times smaller.

b. 1000 times larger d. 100 times larger

______ 20 What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL?

a. 86 mL c. 2.4 x 10 mLb. 1.2 x 10 mL d. 42 mL

______ 21 the temperature reading of -14° C corresponds to a Kelvin reading of:

a. 297.6 K c. 287 Kb. -287 K d.259 K

______ 22. Concentrated hydrochloric acid has a density of 1.19 g/mL. What is the mass, in grams

of 2.00 Liters of this acid?

a. 2.38 x 10 g c. 4.20 x 10 gb. 2.38 g d. 4.20 x 10 g

______ 23. A conversion factor:

a. Is equal to 1b. Is a ratio of equivalent measurements.c. Does not change the value of a measurement.d. All of the above

______ 24. Chlorine boils at 239 K . What is the boiling point of chlorine expressed in degrees

Celsius?

a. 93° C c. -61° Cb. 34° C d. -34° C

______ 25. A student measures a volume as 25 mL, whereas the correct volume is 23 mL . What is

the percent error?

a. 0.087 % c. 0.92%b. 8.7 % d. 8.0 %

Problems

26. A cube of gold-colored metal with a volume of 64 cm has a mass of 980 g. The density of pure gold is 19.3 g/cm . Is the metal pure gold?

27. Perform the following operations. Make sure that your answers have the correct number of significant digits.

a. 4.15 cm x 1.8 cm

b.13.00 m – 0.54 m

c.(1.7 x 10 m) x (3.72 x 10 m)

28. Calculate the density of a liquid that has a mass of 14.0 g and a volume of 18.0 cm .

Ch 4

Write the word that describes the concept.

1. The total number of protons and neutrons in the nucleus of an atom.

2. The weighted average mass of the atoms in a naturally occurring sample of an element

3. 1/12 the mass of a carbon-12 atom

4. The number of protons in the nucleus of an element.

5. Atoms with the same number of protons but different numbers of neutrons.

6. Negatively charged subatomic particle

7. The smallest particle of an element that retains its identity in a chemical reaction.

8. A horizontal row of the periodic table

9. Subatomic particle with no charge.

10. Positively charged subatomic particle.

Multiple Choice

______ 11. Which of the following is not a part of Dalton’s atomic theory?

a. All elements are composed of atomsb. Atoms of the same element are alike.c. Atoms are always in motion.d. Atoms that combine do so in simple whole-number ratios.

______ 12. The nucleus of an atom is

a. Negatively charged and has a low densityb. Negatively charged and has a high densityc. Positively charged and has a low densityd. Positively charged and has a high density

______ 13. Dalton theorized that atoms are indivisible and that all atoms of an element are

identical. Scientists now know that

a. Dalton´s theories are completely correct.b. Atoms of an element can have different numbers of protons.c. Atoms are all divisible.d. All atoms of an element are not identical but they all have the same mass.

______ 14. The number of neutrons in the nucleus of an atom can be calculated by

a. Adding together the numbers of electrons and protons.b. Subtracting the number of protons from the number of electrons.c. Subtracting the number of protons from the mass number.d. Adding the mass number to the number of protons.

______ 15. The sum of the protons and neutrons in an atom equals the

a. Atomic numberb. Number of electronsc. Atomic massd. Mass number

______ 16. All atoms of the same element have the same:

a. number of protonsb. number of neutronsc. mass numberd. mass

______ 17. Which of these statements is false?

a. Electrons have a negative charge.b. Electrons have a mass of 1 amuc. The nucleus of an atom is positively charged.d. The neutron is found in the nucleus of an atom.

______ 18. An atom of an element with atomic number 48 and mass number 120 contains

a. 48 protons, 48 electrons, and 72 neutronsb. 72 protons, 48 electrons, and 48 neutronsc. 120 protons, 48 electrons, and 72 neutronsd. 72 protons, 72 electrons, and 48 neutrons

______ 19. How do the isotopes hydrogen-2 and hydrogen-3 differ?

a. Hydrogen-3 has one more electron than hydrogen-2b. Hydrogen-3 has two neutronsc. Hydrogen-2 has three protonsd. Hydrogen-2 has no protons

______ 20. The number 80 in the name bromine-80 represents

a. The atomic numberb. The mass numberc. The sum of protons and electrons.d. None of the above

______ 21. Which of these statements is not true?

a. Atoms of the same elements can have different masses.b. The nucleus of an atom has a positive charge.c. Atoms of isotopes of an element have different numbers of protons.d. Atoms are mostly empty space.

______ 22. Relative atomic masses are measured in

a. Nanograms.b. Gramsc. Angstroms.d. Amus

______23. If E is the symbol for an element, which two of the following symbols represent

isotopes of the same element.

1. E 2. E 3. E 4. E

a. 1 and 2b. 3 and 4c. 1 and 4d. 2 and 3

Problems

24. There are five naturally occurring isotopes of the element zinc. The relative abundance and mass of each are as follows.

Zn = 48.89 % 63. 929 amu

Zn = 27.81%, 65.926 amu

Zn = 4.11%, 66.927 amu

Zn= 18.57%, 67.925 amu

Zn= 0.62%, 69.925 amu

Calculate the average atomic mass of zinc.

25. Complete this table

Atomic Number Mass Number Number of Protons

Number of Neutrons

Number of Electrons

9 10

14 7

21 20

13 27

56 26

26. List the number of protons, neutrons and electrons in each of the following atoms.

Protons Neutrons Electrons

C

Be

Ne

B

S

Ch 5

Write the letter of the concept that best fits the definition

a. Aufbau principal f. energy levelb. Quantum g. Hund´s rulec. Photoelectric effect h. electron configurationsd. Atomic orbitals i. quantum mechanical modele. Pauli exclusion principle j. photons

______ 1. The ways in which electrons are arranged around the nuclei of atoms

______ 2. The ejection of electrons by metals when light shines on them

______ 3. The region around the nucleus of an atom where an electrons is likely to be moving

______ 4. An atomic orbital may describe at most two electrons.

______ 5. The regions within which electrons have the highest probability of being found

______ 6. When electrons occupy orbitals of equal energy, one electron enters each orbital until

all the orbitals contain one electron.

______ 7. The amount of energy required to move an electron fromits present energy level to the

next higher one.

______ 8. Light quanta

______ 9. Electrons enter orbitals of lowest energy first.

______ 10. The modern description of the electrons in atoms.

Multiple choice

______ 11. Bohr´s contribution to the development of atomic structure

a. Was referred to as the “plum pudding model”b. Was the discovery that electrons surround a dense nucleus.c. Was proposed that electrons travel in circular orbits around the nucleus.d. Is the quantum mechanical model.

______ 12. What is the total number of orbitals in the third principal energy level?

a. 1 b. 4 c. 9 d. 16

______ 13. What is the maximum number of electrons allowed in the third energy level?

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

______ 14. What is the maximum number of electrons that can occupy one orbital?

a. 1 b. 2 c. 8 d. 18

______ 15. The electron configuration for fluorine is

a. 1s 2s 3p c. 1s 2s 2p b. 1s 2s 2p d. 1s 2s 2p 3s

______ 16. The first three electrons that enter into p orbitals must have

a. Parallel spins c. low energy levelsb. Opposite spins d. opposite charges

______ 17. The atom whose electron configuration is 1s 2s 2p 3s 3p is

a. B b. Na c. Al d. Ga

______ 18. The configuration for the outermost energy level in Ca is

a. 3s b. 4s c. 2s d. 4s

______ 19. The element having the same s and p configurations for principal energy level 3 as the

element F has for its principal energy level 2 is

a. Na b. Al c. P d. Cl

______ 20. The frequency and wavelength of all waves are

a. Directly related. c. unrelatedb. Inversely related. d. equal

______ 21. The SI unit of cycles per second is called a

a. Photon c. hertzb. Quantum d. hund

______ 22. Among the following groups of atoms, which have the same outer energy level

configurations?

a. H, He c. Mg, Al, Ca, Ga

b. Li, Be, N , Ne d. N, P, As, Bi

______ 23. The wavelength of light with a frequency of 2.50 x 10 s is

a. 1.20 x 10 m c. 1.20 x 10 mb. 8.33 x 10 m d. 8.33 x 10 m

______ 24. Once the electron in a hydrogen atom absorbs a quantum of energy, it

a. Is now in tis ground state c. has released a photonb. Is now in its excited state d. none of the above

Matching

Column A Column B

______ 30. The lowest energy level within which an electron can a. Heisenberg uncertainty

be found principle

______ 31. The height of an electromagnetic wave from the b. wavelength

to the crest

______ 32. It is impossible to know exactly both the velocity and c. ground state

the position of a particle at the same time

______ 33. The number of electromagnetic wave cycles to pass a d. amplitude

Given point per unit of time

______ 34. All matter exhibits wavelike motion e. de Broglie´s equation

______ 35. The distance between the crests of an electromagnetic f. frequency

wave

Problems

31. Write the electron configurations

a. Mg

b. P

c. Br

d. Xe

32. Identify the elements described below.a. Configuration = 1s 2s 2p 3s 3p

b. contains a full second energy level

c. Contains the first d electrond. Contains seven electrons in its fourth energy levele. Contains only two electrons in its fifth energy levelf. Contains three unpaired electrons in its third energy levelg. Contains five electrons in its 3d orbitalsh. Has its outermost electron in 7s

33. What is the frequency of radiation whose wavelength is 6.25 x 10 cm?