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Chemistry 112 > Chem 112 Finals > Flashcards

Chem 112 Finals Flashcards

1
Q

What is Matter?

A

anything that occupies space and has mass, anything made up of atoms.
Any matter that can be identified as a particular “type” is called a “substance”

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2
Q

What is a physical property?

A

characteristics observed without changing basic identity of
substance. The key is that molecular structure of substance is not altered.
e.g. colour, melting point, density
(no new bonds are formed or broken)

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3
Q

What is an intensive property?

A

characteristic not depending on amount of substance
present. They depend on the internal makeup of the substance.
e.g. density, temperature, boiling point of a pure substance

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4
Q

What is an extensive property?

A

characteristics depending on amount of substance
present, e.g. mass, volume, heat content

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5
Q

what is a chemical property

A

any characteristic of a substance that involves ability (or
inability) of substance to react to form other substances. The molecular structure
of substance being studied (reactant) is altered if reaction occurs.
e.g. flammability of carbon in oxygen gas
e.g. non reactivity of Au in hydrochloric acid solution
(new bonds are formed and broken)

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6
Q

what is organic compound

A

-A molecule containing carbon and hydrogen atoms
-May have additional elements, especially oxygen and
nitrogen

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7
Q

what is inorganic compound

A
  • Any molecule that doesn’t match the rules for organic
    compounds!
  • Always exceptions: e.g. H 2CO3 (carbonic acid) is
    considered to be an inorganic compound
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8
Q

constitutional/structural isomer

A

have same molecular formula but different connection scheme for the atoms

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9
Q

isomer

A

same chemicla formula but different structures and properties

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10
Q

enantiomers

A

nonsuperimposable mirror images

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10
Q

stereoisomers

A

same forumla and connectivity but different spatial arrangmements of substituents

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11
Q

diastereomers

A

not enantiomers (cis and trans isomers)

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12
Q

Boyles Law

A

relationship between gas volume and pressure P1V1=P2V2
(v inversely related to P)

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13
Q

Charles Law

A

relationship between volume and temp V1/T1=V2/T2
(directly related)

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14
Q

Avogardos law

A

relationship between volume and number of moles V1/n1=V2/n2
(directly related)

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15
Q

daltons law of partial pressure

A

each component of a gas mixture exerts a pressure that it would exert if it were in the countainer alone (same n and V)
the total pressure of gases is the sum of the partial pressures of the components mixture

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16
Q

theories of gas

A
  1. mass but no volume
  2. seperated by great distance
  3. collide only fleetingly
  4. no forced b/w molecules
  5. energy remains constant
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17
Q

connection b/w kinetic energy and pressure

A
  • pressure is due to collision of gas molecules
  • higher molecular speed - higher pressure
  • higher collision frequency - higher pressure
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18
Q

diffusion

A

lower concentration zone is filled with other gases; collisions occur during mixing

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19
Q

effusion

A

lower concetration zone is empty(vacuum); gas moves without collisions

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20
Q

Grahms Law

A

light molecules move more rapidly than heavy molecules in diffusion and effusion

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21
Q

what is thermochemistry

A
  • study of heat effects that accompany chemical reactions
  • concerened with the interconversion of heat, work and energy
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22
Q

open system

A

have boundaries that permit the flow of matter and energy in our out of it (e.g. car engine, beaker)

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23
Q

closed system

A

boundaries impermeable to the flow of matter, but energy can still flow in and out (e.g. covered erlenmeyer flask)

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24
isolated system
boundaries impermeable to the flow of matter and energy (e.g. thermos)
25
kinestic energy
energy of motion
26
potential energy
energy is stored - by position, wihtin a spring, wihtin a chemical bond, within the particels of nucleus
27
energy exchnage
energy is exchanged between the system and its surroundings through heat and work q>0 system gains heat w>0 system gains energy
28
exothermic
system releases heat q<0 (*
29
endothermic
system gains heat q>0
30
first law of thermodynamics
energy is not created nor destroyed during chemical or physical processes
31
internal energy
total amount of kinetic and potential energy a system posesses. only deopends on amount of energy in the beginning and end of system
32
contributions of internal energy
- translational kinetic energy - molecular mrotaiton - bond vibration - intermolecular attractions - chemical bonds - electron motions - nuclear energy
33
standard state
st6ate of a material at a defined set of conditions
34
standard reaction enthalpy
enthalpy change of a reaction when all reactants and products are in their standard states
35
Hess's Law
if a reaction csn be expressed as a series of steps, then the deltaH for the overall reaction is the sum of the deltaH values for each step
36
spontaneous process
process that occurs in a system left to itself. once started no action from outside is necessary to make th eprocess ocntinue
37
nonspontaneous process
will not occur unless some external action is continuously applied
38
black body radiation
energy is quantisized: system can only absorb or emit energy in discrete amounts called quanta
39
photoelectric effect
when light strikes the surface of certain metals, electrons are ejected
40
atomic emission spectra
if we heat up atoms, they emit light but only at discrete frequencies. is discontinuous and each element has is own distinctive line spectrum. radiation is emitted or absorbed by a transition of the electron from one quentum state to another
41
heisnebergs uncertainty principale
ther eis uncertainty in measuring a variable of a particle
42
bohrs atomic model
1. electrons move in circular orbits around the nucleus 2. orbits have fixed radius and energy levels 3. an electron can move between orbits by accepting or emitting discrete amounts of energy
43
n quantum number
-principale quantum number -principale shell determines energy of orbital
44
l quantum number
- orbital angular momentum quantum number - sub shell - determines shape of orbital
45
ml quantum number
- magnetic quantum number - orbital - determines orientation of orbital
46
multielectron atoms
the repulsion between eletrons means that they stay away from one another in a multieletron atom. electrons in orbitals closer to numcelus affect energy o fhigher orbital electrons
47
penetration
ability of electrons in s-orbitals that allows them to get close to nucleus
48
diamagnetic atoms or ions
all electrons are paired, weakly repelled by a magnetic field
49
paramagnetic atoms or ions
unpaired electrons, attracted to an external magentic feild. the more unpaired electrons present, the stronger this attraction is.
50
polar covalent bonds
covalent bond in which the electrons are not shared equally between 2 atoms
51
formal charges
when atoms have not contributed equal # of electrons to the covalent bonds joining them
52
resonance structure
two or more plausible lewis structures contirbute to the correct structure. - must all have same skeletal steucture - cna differ only in how electrons are distributed wihtin structureVS
53
VSEPR theory
electron pairs repel each other, whetehr they are in chemical bonds or lone pairs. electorn pairs assume orientations about an atom to minimize repulsion
54
bond order
whether a covalent bond is single, double, or triple
54
bond length
distance between the centers of two atoms joind by a covalent bond
55
bond energies
quantity of energy required to break one mole of covalent bond in a gaseous species
56
valence bond theory
core electrons and lone pair valence electrosn stay in the same orbital locations as in the seperated atoms, but the bonding electrons do not
57
hybridization of atomic orbitals
transforming pure atomic orbitals into reformulated atomic orbitals for bonded atoms. the new orbitals are called hybrid orbitals. the number of hybrid orbitals equals the number of pure atomic orbitals
58
contructive interference
occurs hwen the throughs and crests are in phase, leading to addition of the two waves
59
destructive intereference
occurs hwen the troughs and crests are out of phase, leading to cancellation of the two waves
60
van der waals forces
all intermolecular forces cause the non-ideal behaviour of gases
61
dipole moment
produced in a molecule when bond dipoles within the molecule do not cancel out
62
polarizability
measures how easily the electron cloud can be perturbed from its average shape. increases with the size of the atom
63
dipole-dipole interactions
interaction between a pair of polar molecules that have permanent dipole. molecules line up with positive end of one molecule aligned with negative end of another. relativeyl strong
64
dipole-induced dipole interactions
interactions can increase interaction of two molecules as the dipole moment on one molecule can induce a dipole in another ono-polar molecule. (ion can also induce dipole)
65
london dispersion forces
- attractive forces even between non polar moelcules. - intantaneous dipole. - relativeyl weak - more polarizable non polar molecules generally have higher BP
66
Hydrogen bonding
- H atom is covalently bonded to a highly electronegative atom (F, N, O)
67
properties of liquids
- cohesive forces (forces b/w like molecules) - adhesive forces (forces b/w unlike molecules) - surface tension (energy or work required to increase the surface area of liquid)

Chemistry 112 (1 decks)

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