Exam 1 Flashcards

What method used by scientists is the systematic approach to the discovery of new information?

a. analytical method

b. hypothetical method

c. chemical method

d. scientific method

e. technological method

Which statement concerning changes in matter is FALSE?

a. a physical change alters the appearance of a substance, but not its identity

b. a chemical change alters the identity of a substance

c. a chemical change always results in the production of a new substance

d. a chemical change is also called a chemical reaction

e. melting and freezing are chemical changes that change both the appearance of the substance as well as the identity of the substance

What statement best describes an intensive property?

a. a property of a substance that does not depend on the quantity of the substance present

b. a property of a substance that depends on the quantity of the substance present

c. a property of a substance that depends on the mass of the substance, but not the volume of the substance

d. a property of a substance that depends on the physical state (solid, liquid, or gas)

e. a property of a substance that changes based on the mass of the material that is present

When hydrogen (H₂) and chlorine (Cl₂) gases are mixed, hydrogen chloride (HCl) is produced. Hydrogen chloride is classified as what type of matter?

a. an element

b. a compound

c. a homogeneous mixture

d. a heterogeneous mixture

e. a solution

A patient weighs 146 pounds and is to receive a drug at a dosage of 45.0 mg per kg of body weight. The drug is supplied as a solution that contains 25.0 mg of drug per mL of solution. What volume of the drug should the patient receive? [1 pound = 454 gram]

a. 0.579 mL

b. 119 mL

c. 362 mL

d. 579 mL

e. 119L

What is the number 0.9050 written in scientific notation using the proper number of significant figures?

a. 0.9x10⁴

b. 9x10^-1

c. 9.05x10^-1

d. 9.050x10⁴

e. 9.050x10^-1

How should the result of the calculation below be reported using scientific notation and the proper number of significant figures?

(4.3169x10⁴)/(2.02x10³) = ?

a. 2.14 x10¹

b. 2.1371x10¹

c. 2.14x10²

d. 2.14x10⁷

e. 2.1370x10⁹

Which physical property of an astronaut will change depending on whether he or she is on Earth or in orbit?

a. mass

b. weight

c. volume

d. all would change

e. none would change

What is the basic unit of volume in the metric system?

a. milliliter

b. cubic centimeter

c. liter

d. gram

e. millimeter

Which temperature would feel the hottest?

a. 100 Celsius

b. 100 Fahrenheit

c. 100 Kelvin

d. All temperatures would feel equally hot

What is the density of a solid object that has the following measurements?

mass = 189.6 g; length = 9.80 cm; width = 46.6 mm; height = 0.111 m

a. 0.267 g/mL

b. 0.374 g/mL

c. 2.67 g/mL

d. 3.74 g/mL

e. 50.7 g/mL

In which state does matter have an indefinite shape and definite volume?

a. solid

b. liquid

c. gas

d. All of the choices are correct

e. None of the choices are correct

Conversion of ice to liquid water or liquid water to steam is an example of what kind of change?

a. physical

b. chemical

c. molecular

d. analytical

e. Both A and B are correct

What are the two classes of pure substances?

a. elements and atoms

b. compounds and molecules

c. element and compounds

d. chemical and physical

e. homogeneous and heterogeneous

Which statement concerning the classification of matter is FALSE?

a. a pure substance is composed of only one type of component

b. an element is a pure substance that cannot be changed into a simpler form of matter by any chemical reaction

c. all matter is either pure substance or a compound

d. a compound is a pure substance made up of two or more different elements combined in a definite, reproducible way

e. a mixture is the physical combination of two or more pure substances in which each substance retains its own identity

What kind of change always results in the formation of new materials?

a. molecular

b. exothermic

c. endothermic

d. physical

e. chemical

Which one of the following is an example of a pure substance?

a. ethyl alcohol

b. sugar water

c. salt and pepper

d. milk

e sand

What Celsius temperature corresponds to -4.6 degrees Fahrenheit?

a. -20 Celsius

b. -20.3 Celsius

c. -23.0 Celsius

d. -10.9 Celsius

e. -68.4 Celsius

How many cm are in 3.5 x 10^-2 km?

a. 3.5 x 10^-1cm

b. 3.5 x 10^-7cm

c. 3.5 x 10²cm

d. 3.5 x 10⁵cm

e. 3.5 x 10³cm

What is the value of the mass number in the isotope ¹³¹ ₅₃I?

a. 53

b. 78

c. 126.9

d. 131

e. 184

when a neutral atom gains one or more electrons, what type of particle is formed?

a. an anion

b. an isotope

c. a proton

d. a positron

e. a cation

In modern atomic theory, Bohr's orbits are replaced by atomic orbitals. What is an atomic orbital?

a. a circular pah around the nucleus travelled by an electron

b. a dense, positively charged region of space at the center of an atom

c. a region of space within an atom where there is a high probability of finding an electron

d. the outermost principle energy level in an atom

e. the lowest energy arrangement of electrons in an atom

What are the columns of elements on the periodic table called?

a. groups

b. shells

c. periods

d. metals

e. rows

Which statement concerning the elements fluorine, chlorine, bromine, and iodine is FALSE?

a. they are all halogens

b. they all have the same electron configuration

c. they are all nonmetals

d. they are all representative elements

e. they all have the same number of valence electrons

What is the general name given to the elements of Group 1A (1)?

a. halogens

b. alkali metals

c. alkaline earth metals

d. noble gases

e. metalloids

What are valence electrons?

a. the electrons located in the nucleus of an atom

b. the interior electrons, located closest to the nucleus

c. the outermost electrons in an atom

d. the electrons with the lowest energy in an atom

e. the total number of electrons in an atom

What requirement must be met in order for two electrons to coexist in the same orbital?

a. the electrons must have different energies

b. the electrons must have the same spin

c. the electrons must have opposite charges

d. the electrons must be in different principle energy levels

e. the electrons must have opposite spins

In nature, the element neon exists as three different isotopes: Ne-20, Ne-21, and Ne-22. Which isotope would be the most abundant in a sample of neon?

a. Ne-20

b. Ne-21

c. Ne-22

d. All isotopes would be equally abundant

e. It is impossible to determine

How many valence electrons are present in a chloride ion, Cl^-?

a. 5

b. 7

c. 8

d. 17

e. 18

Which ion is NOT isoelectronic with Ar? The electron configuration of Ar is shown below.

Ar 1s² 2s² 2p⁶ 3s² 3p⁶

a. Cl^-

b. K⁺

c. Br^-

d. Ca²⁺

e. S^2-

The ground state electron configuration of a sulfur atom is shown below. What is the electron configuration of the ion S^2-?

a. 1s² 2s² 2p⁶ 3s⁰ 3p⁴

b. 1s² 2s² 2p⁶ 3s² 3p⁶

c. 1s² 2s² 2p⁶ 3s² 3p²

d. 1s² 2s² 2p⁶

e. 1s² 2s² 2p⁶ 3s³ 3p⁵

The element carbon forms the basis of study in Organic Chemistry. Which statement about the element carbon is FALSE?

a. Carbon is a period 2 element

b. Carbon is a group 14 element

c. Carbon is a nonmetal

d. Carbon atoms have six valence electrons

e. Carbon atoms have six protons

In a neutral atom, what number equals the number of electrons?

a. atomic number

b. mass number

c. mass number minus the atomic number

d. Both A and C are correct

e. None of the choices are correct

How many neutrons are present in an atom of the isotope ⁷ ₃Li?

a. 3

b. 4

c. 7

d. 10

e. None of the choices are correct

How many orbitals are in an s sublevel? How many in a p sublevel?

a. s: 1, p: 2

b. s: 2, p: 3

c. s: 1, p: 3

d. s: 2, p: 6

e. s: 3, p: 3

What Group IA (1) ion has the electronic arrangement shown below?

1s ² 2s ² 2p⁶

a. lithium ion

b. sodium ion

c. potassium ion

d. magnesium ion

e. calcium ion

Which isotope of hydrogen has two neutrons?

a. hydrogen-1

b. hydrogen-2

c. hydrogen-3

d. deuterium

e. H₂

Which of the following accounts for the fact that chlorine has an atomic mass of 35.45 amu rather than a whole number?

a. isotopes

b. electrons

c. protons

d. radioactivity

e. isomers

Rutherford's experiment, in which alpha particles were aimed at a thin piece of gold, led to what understanding?

a. neutrons existed

b. electrons existed and have a negative charge

c. the number of electrons can be determined by the mass number and atomic number

d. electrons can be promoted to higher energy by absorbing energy

e. apart from a very small nucleus containing the protons, an atom is mostly empty space