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Chem > Exam 1-4 > Flashcards

Exam 1-4 Flashcards

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1
Q

The phase transitions from a liquid to a solid is _______

A

freezing

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2
Q

which of the following of a physical change

A

animal fat melts into a liquid when warmed on the stove

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3
Q

Carbon 12 and carbon 13 are _____; they have different numbers of ______

A

isotopes ; neutrons

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4
Q

EX of an exact number

A

5 goldfish

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5
Q

do neutrons and electrons have the same number?

A

yes

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6
Q

Gluecose in C6H12O6. An individual glucose _____ is made up of ______. Glucose is a(n) ______

A

molecule; atoms; compound

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7
Q

A drink made of water, sugar, grape flavoring, and purple food coloring where everything is throughly mixed up is _______.

A

A homogeneous mixture

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8
Q

A proton has ____ charge and is located _____. It has approximately the same mass as a(n) ______.

A

a positive; in the nucleus; neutron

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9
Q

A horizontal row on the periodic table is a _______, and a vertical column is a _______.

A

period; group

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10
Q

Which of the following is NOT a physical property of water?

A

Hydrogen (H2) and oxygen (O2) react to form water.

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11
Q

Fluorine is a _______, lithium is a _______, and boron is a ________

A

nommetal; metal; metalloid

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12
Q

The energy pf a photon is ______ proportional to its wavelength and ________ proportional to its frequency.

A

inverslt; directly

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13
Q

The absorbance of infrared (IR) light by gases such as carbon dioxide make these gases _________

A

greenhouse gases

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14
Q

If you add a cup of sugar to a quart of water in the process of making Kool Aid, you’ve prepared a _____ with sugar as the _____ and water as the _______

A

solution; solute; solvent

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15
Q

Which of the following is NOT a major source of CO2 in the atmosphere today?

A

Emissions from carbonated beverages

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16
Q

What are the products of the reaction of HI with Ba(OH)2

A

BaI2 and water

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17
Q

Combustion reactions ______ heat; they are ______ process

A

release; exothermic

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18
Q

single bond
double bond
triple bond

A

1 sig bond
1 sig bond, 1 pi bond
1 sig bond, 2 pi bond

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19
Q

Which of the following processes has contributed the most to the increasing atmospheric
CO2 concentration in recent years?

A

fossil fuel combustion

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20
Q

A pi bond is formed by the _______ overlap of _______ orbitals.

A

side-by-side; unhybridized p

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21
Q

An exothermic reaction causes the surroundings to.

A

warm up

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22
Q

Greenhouse gases including ________ increase global temperatures because they absorb
____ light.

A

CO2 and CH4; IR

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23
Q

If you add a spoonful of table salt to a pot of water before cooking noodles, you’ve
prepared a _____ with water as the _____ and salt as the _____

A

solution; solvent; solute

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24
Q

A sample of water is being studied. It sits in an open beaker on a lab bench. Which of the
following is true?

A. The water constitutes the thermodynamic system.
B. The beaker plus everything else in the room and in the universe, except the water,
constitute the surroundings.
C. The water plus the beaker are the system.
D. The beaker is part of the system.
E. Both A and B are true

A

E: Both A and B are true

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25
Q

When heat is transferred to the system from the surroundings, the process is said to be
________, and the sign of q is ________

A

endothermic; positive

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26
Q

A O-O bond is _________ and _________ than a O=O bond

A

longer; weaker

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27
Q

The numerical value of an element’s electronegativity represents

A

the ability of an atom in a bond to draw shared electrons to itself.

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28
Q

Why is resonance used to describe some Lewis structures

A

The true structure is an average between the different resonance structures and cannot be
described by a single structure

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29
Q

Which intermolecular force(s) is/are found between molecules of water and ammonia, NH3

A

London dispersion forces, dipole-dipole forces, and hydrogen bonding

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30
Q

Valence bond theory describes how a covalent bond is formed by

A

the overlap of two orbitals, with each orbital containing one electron

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31
Q

When a covalent bond forms between two atoms, the potential energy of the system
_________. To break a bond, energy must be ______

A

decreases; added

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32
Q

If photons in an energy source are changed from microwaves to x-rays, how does the energy of the
photon change

A

The energy of the photon increases

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33
Q

What is the maximum number of electrons that can occupy the n = 2 shell

A

8

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34
Q

In a multielectron atom, which of these subshells has the highest energy

1s, 2p, 4p, 5f, 5d

A

5f

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35
Q

The effective nuclear charge experienced by valence electrons is generally _______ the nuclear
charge due to shielding by the ______

A

lower than; core electrons

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36
Q

atomic radius

A
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37
Q

electron affinity

A
38
Q

A lithium ion has a ____ radius than a lithium atom, and a chloride ion has a _____ radius than a
chlorine atom

A

smaller; larger

39
Q

compound

A

2+ elements in fixed proportions

40
Q

The Lewis symbol for a fluorine atom has ____ dots, and the Lewis symbol for a fluoride ion has
____ dots

A

7; 8

41
Q

The lattice energy for ionic crystals increases as the charge on the ions ________ and the size of the
ions ________

A

increases; decreases

42
Q

What is the name of Mn(CO3)2?

A

manganese(IV) carbonate

43
Q

The compound, P4S10, is used in the manufacture of safety matches. What is its name

A

tetraphosphorus decasulfide

44
Q

empirical formula

A
45
Q

What is the formula for the compound formed by calcium and chlorine

A

CaCl2

46
Q

Which of the following electron transitions causes the emission of a photon with the shortest
wavelength

A

k–>g

47
Q

Which piece of information below cannot be inferred or calculated from the formula for a
chemical substance?

A

The electrical conductivity of the substance

48
Q

The Lewis dot symbol consists of the symbol for the element surrounded by dot(s). What do
the dots represent

A

valence electrons

49
Q

Which of the following statements best describes the location and movement of electrons in an
atom?

A

Electrons have a high probability of being found in regions of three-dimensional space
called orbitals.

50
Q

A 4p subshell consists of ________. A 4p subshell can hold up to ________

A

three orbitals; six electrons

51
Q

Which one of these elements is a transition element?

A. nickel
B. tin
C. sodium
D. sulfur
E. calcium

A

nickel

52
Q

The effective nuclear charge for an atom is less than the actual nuclear charge due to

A

shielding

53
Q

effective nuclear charge

A
54
Q

Which of the following statements correctly compares orbitals in a gold atom

A

A 5p orbital is larger and has a higher energy than a 4p orbital

55
Q

In the modern periodic table, elements are arranged in order of increasing _____

A

atomic number

56
Q

A silicon atom has ______ valence electrons

A

4

57
Q

Which of the following could represent a molecular formula but not an empirical formula?

A. C2H4
B. NaCl
C. CaCl2
D. MgO
E. H2O

A

A: C2H4

58
Q

What is the correct name of Mg3N2

A

magnesium nitride

59
Q

molecular

A
60
Q

Elements with the highest first ionization energies are found in the ________ region of the
periodic table.

A

upper right

61
Q

The group of elements exhibiting the highest electron affinities are ______

A

the halogens

62
Q

What can be said about the relative ionization energies IE1, IE2, etc. of a multi-electron-atom?

A

For carbon, IE5 is substantially larger than IE4

63
Q

Why do main group elements tend to form ions with predictable charges?

A

These elements gain or lose electrons until their electron configuration is the same as
the nearest noble gas

64
Q

How many significant figures are in 0.006570 L

A

4

65
Q

Which of the following represents an exact quantity

A

a student has 2 eyes

66
Q

Which of the following does not have a uniform composition throughout

A

heterogeneous mixture

67
Q

The majority of the volume of an atom is occupied by.

A

electrons

68
Q

Which of the following is a chemical change?

A

EX 1: broiling a steak on a grill

EX 2: turning hair yellow with bleach

69
Q

chemical change

A

change in composition, the og substance does not exist

EX: buring, digestion, oxidation

70
Q

isotopes

A

different # of electrons

71
Q

polymers

A
72
Q

monomers

A
73
Q

sublimation

A

solid –> gas

74
Q

deposition

A

gas –> solid

75
Q

What name is given to the phase transformation by which a solid passes directly into the
gaseous state without passing through an intermediate liquid?

A

sublimation

76
Q

precise results vs. accurate results

A

Accuracy: closeness to experimental measurements to the real value

precision: how close repeated numbers are to each other

77
Q

In the periodic table, the group of elements containing sodium (Na) is called the ______

A

alkali

78
Q

Which statement concerning atomic structure and its representation is true?

A. The nucleus of an atom contains neutrons and electrons.
B. The atomic number of an element is the number of protons in one atom.
C. The mass number of an atom is the number of protons in the nucleus plus the number of
electrons outside.
D. The number of electrons outside the nucleus is the same number of neutrons in the
nucleus.
E. The mass number and the atomic number are the same thing.

A

The atomic number of an element is the number of protons in one atom

79
Q

The majority of elements are ____

A

metals

80
Q

standard state

A
81
Q

Which of the following is NOT a metalloid?

A. Pb
B. B
C. Ge
D. Sb
E. Te

A

A; Pb

82
Q

Which of the following statements about moles is false?

A. 1 mole of sodium has 6.022 × 1023 sodium atoms
B. 1 mole of carbon has the same number of atoms as 1 mole of silver
C. 1 mole of neon has a mass of 20.18 g
D. 1 mole of helium has a mass of 4.003 amu
E. 1 mole of beryllium has a larger mass than 1 mole of lithium

A

1 mole of helium has a mass of 4.003 amu

83
Q

What type of electromagnetic radiation has a frequency of 2.9 x 109 Hz?

A

Microwave
You have version A of the exam. Please bubble A for your exam version.

84
Q

atomic mass

A

protons and nuetrons

85
Q

The volume occupied by an atom is determined by its _______; the atomic mass is determined
by the number(s) of ______

A

electrons; protons and neutrons

86
Q

Camphor is a waxy, soft, white solid with a strong, pleasant odor. If you place a sample of
camphor in a dish on a lab bench and return the next day, the camphor will be gone because of
the process of sublimation. Which of the following statements is true about this process?

A. Sublimation is the conversion of a solid to a liquid.
B. Sublimation is the direct conversion of a solid to a gas without passing through an
intermediate liquid state.
C. Sublimation is the oxidation of camphor into a volatile species.
D. Sublimation and condensation both describe similar processes.
E. Sublimation represents the two-step process of condensation followed by freezing.

A

B. Sublimation is the direct conversion of a solid to a gas without passing through an
intermediate liquid state.

87
Q

Atoms of the same element with different mass numbers are called _______

A

isotopes

88
Q

If a clear hummingbird nectar is prepared by stirring sugar into water, the hummingbird nectar
is a . . .

A. solute.
B. compound.
C. homogeneous mixture.
D. heterogeneous mixture.
E. solvent.

A

C. homogeneous mixture.

89
Q

A sample substance from which state of matter has a constant volume but can adopt the shape
of its container?

A. Liquid
B. Solid
C. Gas
D. Plasma
E. No state of matter has these characteristics.

A

A. Liquid

90
Q

an atomic orbital…..

A

is a fixed pathway traveled by an electron

91
Q
A

Chem (11 decks)

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