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Chem/Phys EXAM 1 > Chapter 2 > Flashcards

Chapter 2 Flashcards

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1
Q

Sub-shell types

A

S, P, D, F

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2
Q

S sub-shell has

A

1 orbital that can hold 2 electrons

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3
Q

P sub-shell has

A

3 orbitals that can hold 6 electrons

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4
Q

D sub-shell has

A

5 orbitals that can hold up to 10 electrons

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5
Q

F sub-shell has

A

7 orbitals that can hold up to 14 electrons

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6
Q

The atomic number identifies

A

The number of protons & electrons

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7
Q

The atomic mass is the

A

Number of protons & neutrons in an atom (sum & is an integer)

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8
Q

The group number identifies the

A

Number of valence electrons

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9
Q

The period number identifies

A

The number of energy levels

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10
Q

What is matter?

A

Anything that has mass & takes up space & does not need to be visible

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11
Q

What is the basic building block of matter?

A

Atoms

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12
Q

Atoms can join to form

A

Molecules

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13
Q

An element

A

Contains only a single kind of atom

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14
Q

Compounds contain

A

2 or more kinds of atoms in a fixed ratio

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15
Q

Atoms are comprised of

A

Protons, neutrons & electrons

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16
Q

Protons are

A

Positively charged

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17
Q

The number of protons is also called the

A

Atomic number & determines the identity of the atom

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18
Q

Neutrons are

A

Neutral

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19
Q

Electrons are

A

Negatively charged

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20
Q

Ions are

A

Atoms or a group of atoms bonded together that have a net electrical charge; charge is obtained by adding or subtracting electrons

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21
Q

Molecules are a

A

Group of atoms chemically bonded together into a discrete unit by covalent bonds & are electrically NEUTRAL

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22
Q

Ionic compounds contain

A

Positively charged ions & negatively charged ions

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23
Q

Ionic compounds are

A

Not molecules

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24
Q

Physical change occurs

A

Without changing the chemical makeup of the substance undergoing the changes (ex;melting)

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25
Q

Chemical changes always result in the formation of

A

Chemically different substances

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26
Q

A physical property can be

A

Observed or measured without changing the chemical makeup of the substance

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27
Q

Which 2 categories do physical properties fall under?

A

Intensive & Extensive

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28
Q

What is Intensive property

A

Is integral to the material, regardless of how much material there is
ex: color

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29
Q

What is Extensive property?

A

depends on the sample size
ex: volume & mass

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30
Q

A chemical property describes

A

Describes the type of chemical change the material tends to undergo
ex: gases are flammable

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31
Q

What are pure substances?

A

materials that cannot be physically separated into simpler components

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32
Q

A substance can either be a

A

Compound or Element

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33
Q

If a substance is a compound, then

A

It can be chemically separated into its elemental components

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34
Q

Mixtures are comprised of

A

2 or more pure substances

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35
Q

Mixtures can be

A

Resolved into simpler components through physical processes

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36
Q

Homogeneous mixtures are

A

Uniform in chemical & physical properties throughout the sample
ex: NS & Air

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37
Q

A heterogeneous mixture exhibits

A

Distinct phase boundaries between its components
ex: Emesis

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38
Q

A phase boundary is

A

A demarcation where the chemical &/or physical properties of the sample change

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39
Q

Can a substance be both a molecule & an element?

A

Yes

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40
Q

Electrons are bound to the nucleus by

A

The electromagnetic force (attraction of opposite charges)

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41
Q

When protons & neutrons combine to form an atomic nucleus,

A

There is a mass deficit because some of the mass is converted into a binding energy

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42
Q

The mass number can

A

NEVER be smaller than the atomic number

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43
Q

Elements are always

A

Electrically neutral

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44
Q

The number of electrons is

A

Equal to the number of protons in an electrically neutral atom

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45
Q

Isotopes have

A

The same atomic number but a different mass number -or- the same number of protons & a different number of neutrons

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46
Q

Compounds are formed by

A

Bonding atoms together in a fixed ratio

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47
Q

Chemical reactions do not

A

Create, destroy, or change atoms into atoms of other elements; chemical reactions cause atoms to recombine into new substances

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48
Q

What is the law of conservation of mass?

A

No detectable change in the total mass occurs during chemical reactions; during a chemical change, the components of a system are neither created nor destroyed; they simply recombine into new substances

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49
Q

What the is law of definite proportions?

A

Different samples of a pure compound always contain the same elements in the same proportion by mass

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50
Q

What is the Law of Multiple Proportions?

A

Some elements can combine to give more than one compound

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51
Q

Elements must be delivered as

A

Particles (i.e., atoms) rather than a continuous substance

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52
Q

How are elements listed on the periodic tabel?

A

In order of increasing atomic number

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53
Q

Vertical columns are called

A

Groups/Families

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54
Q

Elements in a given group have similar

A

Chemical & physical properties

55
Q

Noble gases are

A

Colorless, odorless & are extremely reluctant to combine with other elements to form compounds

56
Q

Each row is called a

A

Period

57
Q

Periods represent adding electrons to

A

Quantum energy levels in the atom, which are called electron shells

58
Q

Atoms with filled electron shells are

A

Stable

59
Q

Accepting additional electrons is called

A

An Anion (negative charge)

60
Q

What are the atomic weights?

A

Are weighted averages of the atomic masses of the naturally occurring isotopes of that element

61
Q

Characteristic of metals on the periodic table

A

Shiny luster

Ductile

Malleable

Good Conductors

React chemically to form cations by giving away electrons

62
Q

Nonmetals tend to form

A

Anions & are brittle

63
Q

What is a well-known semi-conductor?

A

Silicon

64
Q

Most elements are

A

Solids under normal conditions

65
Q

Molecular compounds are comprised of

A

Only nonmetals

66
Q

Ionic compounds are almost always comprised of a

A

Metal & a nonmetal

67
Q

What is an ion?

A

An atom or a group of atoms with a charge

68
Q

Ionic compounds consists of ions & are

A

Held together by ionic bonds, or the attraction of the oppositely charged ions

69
Q

In the solid state, ionic compounds form

A

Crystalline lattices, in which all the cations are attracted to all the neighboring anions

70
Q

Ionic compounds are sometimes referred to as

A

Salts

71
Q

A salt is produced by

A

The reaction of an acid & a base

72
Q

Representative metals almost always form

A

Cations in which the ionic charge equals the group number

73
Q

Most transition metals

A

Form more than one cation

74
Q

Polyatomic ions are formed from

A

2 or more nonmetal atoms that are bonded together in a way that results in a net electrical charge

75
Q

Compounds must be

A

Electrically neutral

76
Q

The net charge on an ionic compound must be

A

Zero

77
Q

Compounds that have a strong tendency to absorb water are called

A

Hygroscopic

78
Q

The anhydrous form of a compound that has a strong tendency to absorb water can

A

Be used as a desiccant

79
Q

Desiccants scavenge the last

A

Traces of water from a system

80
Q

Electricity is described as the

A

Flow of charged particles under the influence of an electric field

81
Q

An electrolyte is a

A

Substance that dissolves in water to give a solution that conducts electricity

82
Q

A nonelectrolyte is a

A

Substance that dissolves ion water to give a solution that does not conduct electricity

83
Q

Molecular compounds are

A

Nonelectrolytes, unless they have acid or base properties

84
Q

When ionic compounds dissolve in water, they mostly

A

Separate into ions that freely & independently move around; the solution will conduct electricity

85
Q

Water is a

A

nonelectrolyte

86
Q

Water is a molecular substance because

A

It is a compund of nonmetals

87
Q

Pure water is a

A

Nonelectrolyte & is a very poor conductor of electricity

88
Q

Stoichiometry includes

A

The calculations that relate amounts of reactants & /or products in a chemical reaction

89
Q

Moles are a quantity of material, analogous toa dozen & is the

A

Amount of substance that contains exactly as many particles as there are in exactly 12g of carbon-12

90
Q

Mole number is often called

A

Avogadro’s number thats equal to 6.02 x 10 to the 23

91
Q

The molar mass of an element is equal to

A

Its atomic mass

92
Q

For molecules, the molar mass is

A

Equal to the sum of the masses of the component atoms

93
Q

Where is the mass number/atomic mass number located?

A

The bottom number in the periodic taable

94
Q

What are isotopes?

A

Same number of protons but different number of neutrons

95
Q

What are the outermost shells of electrons called?

A

Valence electrons

96
Q

What is involved in molecular bonding?

A

The valence electrons

97
Q

Molecular bonding may occur

A

By direct sharing of electrons or by thermodynamic interaction

98
Q

What are the 2 types of bonds?

A

Covalent & Electrostatic

99
Q

What is it called when atoms of differing elements bond?

A

Compounds

100
Q

The physical sharing of electrons between atoms is called a

A

Covalent bond

101
Q

What are stronger than electrostatic bonds?

A

Covalent Bonds

102
Q

Electrostatic bonding may include

A

Ion-Ion

Ion-Dipole

Dipole- Dipole

103
Q

Which is the strongest electrostatic bond?

A

Ion to Ion

They are not directions & occur anywhere

104
Q

Molecules with ionic bonds have

A

Higher melting & boiling points

105
Q

Ion to dipole bonds only have

A

Partial charges

106
Q

An uneven distribution of charges creates a

A

Dipole

107
Q

Which is the weakest of ALL molecular bonds?

A

London forces

108
Q

Lewis structures are

A

Dots or lines that show valence electrons; only the outer shell is depicted

109
Q

What are isomers?

A

Molecules that have the SAME chemical formula but DIFFERENT structures

110
Q

What is the same in isomers?

A

The number & type of atoms & bonds, but the arrangement of the atoms are different

111
Q

Isomers can be

A

Structural or Stereoisomers

112
Q

What are structural isomers?

A

Have the same molecular formula, but their atoms are located in different places

113
Q

Structural isomers are truly

A

Different molecules with differing physical & chemical properties

114
Q

What are stereoisomers?

A

Have similar geometric arrangement of atoms but differ in their spatial position

115
Q

Stereoisomers can be

A

Enantiomers or Diastereomers

116
Q

What are enantiomers?

A

Mirror images of one another & CANNOT BE superimposed

Have similar chemical & physical properties

Optically active & can rotate polarized light in a clockwise fashion (+/dextro) or counterclockwise (-/leva)

117
Q

What are diastereomers?

A

NOT mirror images & may have differing physical & chemical properties

118
Q

What is bond energy?

A

The amount of energy needed to make or break a bond

119
Q

Energy is released when

A

A bond is formed

120
Q

Energy is consumed when

A

A bond is broken

121
Q

What possess greater bond energy?

A

Short bonds like covalent bonds

122
Q

What happens when molecular bonds are broken?

A

New molecular bonds are formed & energy is released

123
Q

Bond energies are measured as

A

An enthalpy change

124
Q

What is Enthalpy?

A

The total amount of energy possessed by a system (system can be on an atomic or macroscopic scale)

125
Q

The Enthalpy of a system is the

A

Total of all kinetic & potential energy

The stored/potential energy includes its height in relation to the force of gravity & the energy stored in the bonds of its molecules, atoms & even subatomic particles

126
Q

Change of energy is

A

Easier to measure rather than total energy (enthalpy)

127
Q

What is mass?

A

Total of all matter in an object- the sum of the mass of all the electrons, protons & neutrons

128
Q

What is weight?

A

The total effect of gravity pulling on all the electrons, protons & neutrons

129
Q

What is a Dyne?

A

1/1000 of a newton

The force required to move 1g of weight 1cm/sec

130
Q

When are Dynes used

A

To calculate SVR & PVR

131
Q

An EKG is an example of a

A

Vector

132
Q

Mass Spectrometry is used

A

In anesthetic gas analysis

(ionized gas molecules)

133
Q

Identification of a gas is based on

A

The amount of deflection

134
Q
A

Chem/Phys EXAM 1 (3 decks)

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