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Quarterlies 3 sala ni ni Pinkyyyy nga naay exam > Gen Chemistry > Flashcards

Gen Chemistry Flashcards

1
Q

Kinetic Theory of Matter

A
  • All matter is made up of tiny particles
  • All particles of one substance are the same
  • Different pure substances are made of different particles
  • Particles are always moving
  • There are attractive forces between particles
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2
Q

Kinetic Molecular Theory of Gas

A
  • The size of the particles is too small compared to the distances between them
  • Gas particles are constantly moving
  • Gas particles do not attract nor repel each other
  • The average kinetic energy of gas particles increases with temperature
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3
Q

Kinetic Molecular Theory of Solids and Liquids

A
  • Liquids and solids have less internal energy to move molecules, making them denser compared to gases
  • The molecules in a liquid are close enough to slide past one another and be slightly compressible, which gives the liquid the ability to assume the shape of its container
  • The molecules of a solid are held rigidly at fixed positions and have little freedom to move. Thus, solid is generally incompressible and has a definite volume and shape
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4
Q
  • attractive forces between molecules; responsible for keeping matter in solid or liquid phases
  • force which keeps molecules together
A

Intermolecular Force

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5
Q

Types of Intermolecular Forces of Attraction

A
  • Dispersion forces
  • Dipole-dipole
  • Hydrogen bond
  • Ion-Dipole
  • Dipole-Induced Dipole
  • Ion-Induced Dipole
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6
Q

attractive forces between polar molecules; uneven sharing of electrons between atoms sharing a covalent bond causes one to be partially positive and the other partially negative

A

Dipole-dipole Force

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7
Q

strong type of dipole-dipole interaction; occurs when molecules interact through dipole-dipole interactions between hydrogen atoms in a polar bond and an electronegative atom.

A

Hydrogen Bond

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8
Q

arises in part from high electronegativity of nitrogen, oxygen, and fluorine

A

Hydrogen Bonding

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9
Q

result from the formation of two temporary dipoles

A

London Dispersion Forces

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10
Q

 results in the interactions between a polar molecule and an ion.

A

Ion-Dipole Force

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11
Q

 tendency of an electron cloud to distort

A

Polarizability

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12
Q

is a force between nonpolar and polar molecules

A

Dipole Induced Dipole

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13
Q

resistance of a liquid to flow

A

Viscosity

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14
Q

an attraction between unlike molecules

A

Adhesion

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15
Q

intermolecular attraction between like molecules

A

Cohesion

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16
Q

broader term that includes evaporation and also boiling

A

Vaporization

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17
Q

gaseous state of a substance which is normally a liquid or solid at room temperature

A

Vapor

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18
Q

substances that evaporate readily

A

Volatile Substances

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19
Q

equilibrium pressure of a vapor above its liquid (or solid), or the pressure of the vapor resulting from evaporation of a liquid above a sample of the liquid in a closed container

A

Vapor Pressure

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20
Q

temperature at which its vapor pressure equals atmospheric pressure.

A

Boiling Point

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21
Q

a simplified representation of valence electron in an element or in a molecule

A

Lewis Dot Structure

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22
Q

refers to the tendency of atoms to prefer to have eight electrons in the valence shell

A

Octete Rule

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23
Q

represents electron shells that are located around the nucleus

A

Energy Level

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24
Q

shows the most probable pathway of an electron that is in motion around the nucleus

A

Orbitals

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25
Q

 a style of notation that depicts the electron distribution and electron spin within orbitals of an atom

A

Orbital Diagram

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26
Q

states that electrons fill lower energy atomic orbitals before filling higher-energy ones

A

Aufbau Principle

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27
Q

states that two electrons in the same orbital must have opposite spin

A

Pauli’s Principle

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28
Q

states that every orbital in a sub level is singly occupied with one electron before any one orbital is doubly occupied

A

Hund’s Principle

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29
Q

Strongest Bond

A

Ionic Bond

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30
Q

The smaller the ion the bigger the attraction

A

The smaller the ion the bigger the attraction

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31
Q

HCI is

A

Dipole Dipole

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32
Q

HN, HO, HF are

A

Hydrogen bonds

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33
Q

intermolecular forces that involves all molecules regardless of polarity

A

London Dispersion

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34
Q

Which of the following is not an intermolecular force?

Dipole Dipole
Covalent Bonding
Hydrogen Bonding
London Dispersion Force

A

Covalent bonding

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35
Q

What type of IMF is present in all substances, regardless of polarity?

A

London dispersion force

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36
Q

Which of the following is the strongest intermolecular force?

Ion-dipole
Ion-induced dipole
Hydrogen bonding
London Dispersion Force

A

Ion-dipole

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37
Q

What type of intermolecular force present in HF?

A

Hydrogen bonding

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38
Q

Which of the following has the highest boiling point?

H2
NH3
N2
O2

A

NH3

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39
Q

Which of the following intermolecular force present in HCl?

Dipole-dipole
Hydrogen Bonding
London Dispersion Force

A

Dipole-dipole

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40
Q

What explains the very high melting and boiling point of water?

A

Strong hydrogen bonds between water molecules.

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41
Q

Which of the following is TRUE about dipole-dipole forces?

It is an attractive force between nonpolar molecules

It is an attractive force between polar molecules

It is an attractive force between ionic compounds

it is an attractive force between polar and nonpolar molecules

A

It is an attractive force between polar molecules

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42
Q

Which of the following statement is TRUE about the ion-dipole interaction?

The bigger the size of son, the bigger the attraction

The smaller the size of ion, the bigger the attraction

The higher the frequency of dipole moment, the lower the possibility of attraction

The lower the frequence of dole moment hnher the nonbity of attraction

A

The smaller the size of ion, the bigger the attraction.

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43
Q

Which of the following is FALSE about KMT of solids and liquids?

Solid are held rigidly at fixed positions and have little freedom to move.

Solids have the ability to assume the shape of its container.

Liquids and solids have less internal energy compared to gases

Liquids are close enough to slide past one another and be slightly compressible.

A

Solids have the ability to assume the shape of its container.

44
Q

Hydrogen bonding occurs when hydrogen is bonded to N, O, or F. Which of the following has hydrogen bonding?

CBr4

NO2

H2S

NH3

A

NH3

45
Q

Does H2O have hydrogen bonding?

A

yes

46
Q

Does CH4 have hydrogen bonding?

A

no

47
Q

Which is the second strongest intermolecular force, after hydrogen bonding?

Dipole-dipole

London dispersion

lon-induced dipole

Dipole-induced dipole

A

Dipole dipole

48
Q

Which of the following is TRUE about ionic bonding

Transfer of protons

Transfer of electrons

Sharing of protons

Sharing of electrons

A

transfer of electrons

49
Q

It is a property of liquid to resist an external force and assume a lesser surface area.

A

surface tension

50
Q

It is the pressure exerted by its vapor when in equilibrium with its liquid or solid

A

Vapor Pressure

51
Q

Which of the following is TRUE about viscosity

Tendency of a liquid to flow

Liquid’s resistance to flow

pressure that equalizes the atmospheric pressure

Boiling point

A

Liquid’s resistance to flow

52
Q

If a liquid has high viscosity, it means that…

A

Strong intermolecular force

53
Q

Which of the following is the most viscous substance?

water

soap

water strider

Honey

A

Honey

54
Q

The attractive force between water molecules.

A

Cohesiveness

55
Q

The attractive force between water molecules and non-water molecule

A

Adhesiveness

56
Q

The tendency of a water molecule to move upward

A

Capillary action

57
Q

Which of the following is TRUE about attractive force in cohesion?

particles of the same substance

particles of both the same and different substances

particles of a different substance

A

particles of the same substance

58
Q

Which of the following is TRUE about capillary action?

property of water that allows ice to float on the surface of liquid water

property of water that allows water to move up a thin tube

property of water that allows it to dissolve polar substances

A

property of water that allows water to move up a thin tube

59
Q

Liquids with weak intermolecular forces

A

easily evaporate

60
Q

Which of the following is true about the strength of intermolecular forces in liquids?

different temperatures

different equilibrium vapor pressure

the same equilibrium vapor pressure

A

different equilibrium vapor pressure

61
Q

Why does ice float?

A

As water freezes, it expands and its density decreases.

62
Q

What is the best explanation for an insect walking across the surface of the water?

The insects’ feet are non-polar, so they are repelled by the polar water molecules and are pushed away from the water’s surface

The insects are light enough so that they do not break the hydrogen bonds holding the water molecules together

The insects are small enough to see the individual water molecules, so they are able to step carefully from one molecule to the next

A

The insects are light enough so that they do not break the hydrogen bonds holding the water molecules together

63
Q

Why water is considered as universal solvent?

A

Dissolves most substance

64
Q

It is a classification of solid that lacks an orderly lattice structure

A

amorphous

65
Q

Which of the following represent a crystalline structure of solid?

molecular
atomic
ionic
all of these

A

all of these

66
Q

It is a type of solid that is conductive.

A

metallic

67
Q

It is a type of solid that is held together by dispersion forces.

A

nonbonding

68
Q

It is a type of solid that is held together by covalent bonds.

A

network covalent

69
Q

It is a type of solid that has molecules as composite units

A

molecular

70
Q

an example of this type of solid is diamond and graphite, both made of carbon atoms.

A

network covalent

71
Q

These solids are typically poor conductors with low melting points

A

molecular

72
Q

NaCl is an example of what type of solid?

A

ionic

73
Q

These solids have particles arranged in a repeating pattern

A

crystalline lattice

74
Q

Covalent Bonding

A

Sharing of electrons

75
Q

Convex

A

Adhesive

76
Q

Concave

A

Cohesive

77
Q

have atoms that are arranged in a regular structure.

A

Crystalline Solids

78
Q

atoms arranged in a repeating patter that forms 3 dimensional networks

A

Crystalline Lattice

79
Q

basic building block of a crystal lattice

A

Unit Cell

80
Q

have atoms that are arranged randomly.

A

Amorphous

81
Q

A crystalline solid has high packing efficiency inside a unit cell. This means that its atoms are found closer to each other compared to the atoms in an amorphous solid.
Crystalline solids have narrow melting point range and high heat of fusion while amorphous solids have wide melting point range and low heat of fusion.

A
82
Q

defined as the temperature and pressure condition under which its molecules will have sufficient energy and freedom to overcome the intermolecular forces that keep them attracted to each other.

A

Solid Melting Point

83
Q

is the amount of energy change needed to increase the low internal energy of a solid to melt it.

A

Heat Fusion

84
Q

Held by intermolecular forces
Relatively soft
Low melting point
Composite Units are molecules

A

Molecular (Ex. Sulfur)

85
Q

Held by strong electro statistic forces
Hard and brittle
High melting point
Composite units are cations and anions

A

Ionic (E.x Table Salt)

86
Q

Have neutral atoms forming their unit cells

A

Atomic

87
Q

London dispersion forces
Soft
Low melting points

A

Non-bonding (Ex. Mineral Graphite, Pure Solid Xenon

88
Q

Metallic bonding
Excellent conductors
High melting point
Unit cells consist of metal ions
Metallic solids have delocalized electrons over the whole solid

A

Metallic Solids (Ex. Copper)

89
Q

Covalent bonding
Generally hard
Melting point depends on crystal structure

A

Network Covalent Bonds (Ex. Quartz)

90
Q

energy required to separate the ions of a crystal into its components

A

Lattice Energy

91
Q

Ionic solids that have multiple charges and smaller sizes have higher lattice energy making them harder to dissociate.

A
92
Q

calculating lattice energy through steps involving the energy changes during the formation of the solid: vaporization of the metal (atomization), ionization of the metal, gain of electrons by the nonmetal, and the overall heat or enthalpy of formation.

A

Born-Haber-Fajans (Born-Haber) Cycle

93
Q

gaps or irregularities in the unit cell of ionic crystals

A

Crystal Defects

94
Q

there is a missing pair of ions in the lattice

A

Schottky Defect

95
Q

there are misplaced ions

A

Frenkel Defect

96
Q

when one of the ions are replaced by a foreign ion

A

Substitutional Defect

97
Q

 interconversion of states of matter

A

Phase Change

98
Q

energy needed to vaporize 1 mole of a liquid

A

Heat Vaporization

99
Q

graph summing up the interconversion of states at a specific temperature and pressure

A

Phase Diagram

100
Q

corresponds to the pressure and temperature where the 3 states of water coexist

A

Triple Point

101
Q

 lies at the end of the liquid-gas boundary

A

Critical Point

102
Q

state of water that have conditions beyond the critical point, which exhibits properties of both a gas and liquid.

A

Supercritical fluid

103
Q

All matter is made up of _______

A

tiny particles

104
Q

All particles of one substance are ________

A

the same

105
Q

Different pure substances are made of _________

A

different particles

106
Q

Particles are always ______

A

moving

107
Q

There are _______ between particles

A

attractive forces

Quarterlies 3 sala ni ni Pinkyyyy nga naay exam (8 decks)

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