Gen Chemistry Flashcards
(107 cards)
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
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
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
4
Q
- attractive forces between molecules; responsible for keeping matter in solid or liquid phases
- force which keeps molecules together
A
Intermolecular Force
5
Q
Types of Intermolecular Forces of Attraction
A
- Dispersion forces
- Dipole-dipole
- Hydrogen bond
- Ion-Dipole
- Dipole-Induced Dipole
- Ion-Induced Dipole
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
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
8
Q
arises in part from high electronegativity of nitrogen, oxygen, and fluorine
A
Hydrogen Bonding
9
Q
result from the formation of two temporary dipoles
A
London Dispersion Forces
10
Q
results in the interactions between a polar molecule and an ion.
A
Ion-Dipole Force
11
Q
tendency of an electron cloud to distort
A
Polarizability
12
Q
is a force between nonpolar and polar molecules
A
Dipole Induced Dipole
13
Q
resistance of a liquid to flow
A
Viscosity
14
Q
an attraction between unlike molecules
A
Adhesion
15
Q
intermolecular attraction between like molecules
A
Cohesion
16
Q
broader term that includes evaporation and also boiling
A
Vaporization
17
Q
gaseous state of a substance which is normally a liquid or solid at room temperature
A
Vapor
18
Q
substances that evaporate readily
A
Volatile Substances
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
20
Q
temperature at which its vapor pressure equals atmospheric pressure.
A
Boiling Point
21
Q
a simplified representation of valence electron in an element or in a molecule
A
Lewis Dot Structure
22
Q
refers to the tendency of atoms to prefer to have eight electrons in the valence shell
A
Octete Rule
23
Q
represents electron shells that are located around the nucleus
A
Energy Level
24
Q
shows the most probable pathway of an electron that is in motion around the nucleus
A
Orbitals
25
a style of notation that depicts the electron distribution and electron spin within orbitals of an atom
Orbital Diagram
26
states that electrons fill lower energy atomic orbitals before filling higher-energy ones
Aufbau Principle
27
states that two electrons in the same orbital must have opposite spin
Pauli’s Principle
28
states that every orbital in a sub level is singly occupied with one electron before any one orbital is doubly occupied
Hund’s Principle
29
Strongest Bond
Ionic Bond
30
The smaller the ion the bigger the attraction
The smaller the ion the bigger the attraction
31
HCI is
Dipole Dipole
32
HN, HO, HF are
Hydrogen bonds
33
intermolecular forces that involves all molecules regardless of polarity
London Dispersion
34
Which of the following is not an intermolecular force?
Dipole Dipole
Covalent Bonding
Hydrogen Bonding
London Dispersion Force
Covalent bonding
35
What type of IMF is present in all substances, regardless of polarity?
London dispersion force
36
Which of the following is the strongest intermolecular force?
Ion-dipole
Ion-induced dipole
Hydrogen bonding
London Dispersion Force
Ion-dipole
37
What type of intermolecular force present in HF?
Hydrogen bonding
38
Which of the following has the highest boiling point?
H2
NH3
N2
O2
NH3
39
Which of the following intermolecular force present in HCl?
Dipole-dipole
Hydrogen Bonding
London Dispersion Force
Dipole-dipole
40
What explains the very high melting and boiling point of water?
Strong hydrogen bonds between water molecules.
41
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
It is an attractive force between polar molecules
42
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
The smaller the size of ion, the bigger the attraction.
43
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.
Solids have the ability to assume the shape of its container.
44
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F. Which of the following has hydrogen bonding?
CBr4
NO2
H2S
NH3
NH3
45
Does H2O have hydrogen bonding?
yes
46
Does CH4 have hydrogen bonding?
no
47
Which is the second strongest intermolecular force, after hydrogen bonding?
Dipole-dipole
London dispersion
lon-induced dipole
Dipole-induced dipole
Dipole dipole
48
Which of the following is TRUE about ionic bonding
Transfer of protons
Transfer of electrons
Sharing of protons
Sharing of electrons
transfer of electrons
49
It is a property of liquid to resist an external force and assume a lesser surface area.
surface tension
50
It is the pressure exerted by its vapor when in equilibrium with its liquid or solid
Vapor Pressure
51
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
Liquid's resistance to flow
52
If a liquid has high viscosity, it means that...
Strong intermolecular force
53
Which of the following is the most viscous substance?
water
soap
water strider
Honey
Honey
54
The attractive force between water molecules.
Cohesiveness
55
The attractive force between water molecules and non-water molecule
Adhesiveness
56
The tendency of a water molecule to move upward
Capillary action
57
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
particles of the same substance
58
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
property of water that allows water to move up a thin tube
59
Liquids with weak intermolecular forces
easily evaporate
60
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
different equilibrium vapor pressure
61
Why does ice float?
As water freezes, it expands and its density decreases.
62
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
The insects are light enough so that they do not break the hydrogen bonds holding the water molecules together
63
Why water is considered as universal solvent?
Dissolves most substance
64
It is a classification of solid that lacks an orderly lattice structure
amorphous
65
Which of the following represent a crystalline structure of solid?
molecular
atomic
ionic
all of these
all of these
66
It is a type of solid that is conductive.
metallic
67
It is a type of solid that is held together by dispersion forces.
nonbonding
68
It is a type of solid that is held together by covalent bonds.
network covalent
69
It is a type of solid that has molecules as composite units
molecular
70
an example of this type of solid is diamond and graphite, both made of carbon atoms.
network covalent
71
These solids are typically poor conductors with low melting points
molecular
72
NaCl is an example of what type of solid?
ionic
73
These solids have particles arranged in a repeating pattern
crystalline lattice
74
Covalent Bonding
Sharing of electrons
75
Convex
Adhesive
76
Concave
Cohesive
77
have atoms that are arranged in a regular structure.
Crystalline Solids
78
atoms arranged in a repeating patter that forms 3 dimensional networks
Crystalline Lattice
79
basic building block of a crystal lattice
Unit Cell
80
have atoms that are arranged randomly.
Amorphous
81
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.
82
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.
Solid Melting Point
83
is the amount of energy change needed to increase the low internal energy of a solid to melt it.
Heat Fusion
84
Held by intermolecular forces
Relatively soft
Low melting point
Composite Units are molecules
Molecular (Ex. Sulfur)
85
Held by strong electro statistic forces
Hard and brittle
High melting point
Composite units are cations and anions
Ionic (E.x Table Salt)
86
Have neutral atoms forming their unit cells
Atomic
87
London dispersion forces
Soft
Low melting points
Non-bonding (Ex. Mineral Graphite, Pure Solid Xenon
88
Metallic bonding
Excellent conductors
High melting point
Unit cells consist of metal ions
Metallic solids have delocalized electrons over the whole solid
Metallic Solids (Ex. Copper)
89
Covalent bonding
Generally hard
Melting point depends on crystal structure
Network Covalent Bonds (Ex. Quartz)
90
energy required to separate the ions of a crystal into its components
Lattice Energy
91
Ionic solids that have multiple charges and smaller sizes have higher lattice energy making them harder to dissociate.
92
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.
Born-Haber-Fajans (Born-Haber) Cycle
93
gaps or irregularities in the unit cell of ionic crystals
Crystal Defects
94
there is a missing pair of ions in the lattice
Schottky Defect
95
there are misplaced ions
Frenkel Defect
96
when one of the ions are replaced by a foreign ion
Substitutional Defect
97
interconversion of states of matter
Phase Change
98
energy needed to vaporize 1 mole of a liquid
Heat Vaporization
99
graph summing up the interconversion of states at a specific temperature and pressure
Phase Diagram
100
corresponds to the pressure and temperature where the 3 states of water coexist
Triple Point
101
lies at the end of the liquid-gas boundary
Critical Point
102
state of water that have conditions beyond the critical point, which exhibits properties of both a gas and liquid.
Supercritical fluid
103
All matter is made up of _______
tiny particles
104
All particles of one substance are ________
the same
105
Different pure substances are made of _________
different particles
106
Particles are always ______
moving
107
There are _______ between particles
attractive forces
