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Chem > Exam 4: Vocab and def > Flashcards

Exam 4: Vocab and def Flashcards

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1
Q

sigma (σ)

A

end-to-end orbital overlap

when sp2 hybrid orbitals on the C atoms overlap

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2
Q

pi (π)

A

side-by-side p orbital overlap

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3
Q

combustion eq

A

____+ O2 –> H2O + CO2

*CO2 ALWAYS has to end up on right side

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4
Q

limiting reactant

A

smallest amount of substance that wont allow you to make more reactant

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5
Q

solutes

A

smaller amount of cmpound

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6
Q

solvent

A

larger amount of compound

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7
Q

M1(V1)= M2(V2)

A

M = concentration
V=volume

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8
Q

Molarity
(concentration)

A

Mol/ Liters (volume)

MoLarity

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9
Q

mass eq

A

Mass= Mol x molar mass

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10
Q

mol eq

A

mass/ molar mass

or

mol = concentration (volume)

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11
Q

Alkaline

A

Produces OH^-

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12
Q

Acid

A

produces H^+

strong acids fully dissolve in water

weak acids partially dissolve in water

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13
Q

heteronuclear diatomic molecules

A

2 diff atoms are IR active

CAN absourb IR

EX: CH4

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14
Q

infared absorption

A

Gases that absorb IR radiation act as greenhouse gases

2 diff atoms or more han 2 atoms absorb IR radiaion

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15
Q

diatomic homonuclear molecules

A

2 IDENICAL atoms CANT absorb IR radiation
ex: Ar or O2

aomic species (noble gases) are IR-INactive

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16
Q

Vocab for eq

___ + ____ —> _____ + ____
Reactants or product?

(s) = ?
(l) = ?
(g) = ?
(aq) = ?

A

left of arrow is reactants
right of arrow is product

(s) = solid
(l) = liquid
(g) = gas
(aq) = aqueous (dissolves in water)

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17
Q

Diatomic elements (2 atoms)

A

H2(g)
N2(g)
O2 (g)
F2(g)
Cl2(g)
Br2(l)
I2 (s)

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18
Q

Combustion reactants (3 types)

A

combustion : a substance burns in the presence of oxygen

combination: two or more reactants COMBINE to form a single product

decomposition: two or more products form FROM a single reactant

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19
Q

theoretical yield

A

calculated amount of product that could form (max)

1) Calculate how much product you could get from each reactant
(separately) and compare those amounts.

2) The smallest amount of possible product is the theoretical yield,
and the amount depends on the limiting reactant.

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20
Q

actual yield

A

measured amount of product actually obtained

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21
Q

Ionic bonds

A

Maal and non-metal dissolve in water

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22
Q

enthalpy

A

another way to measure heat change

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23
Q

ENDOthermic

A

absorbs heat

EX: water getting warmer

heat flows inot system from surrounding
surrounding lose heat

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24
Q

EXOthermic

A

Closed heat

EX: buring log

heat flows out of system to surroundings

makes syrrounding hotter

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25
Q

precipitation

A

2 liquids produce solid

not soluable = will precipaiate

26
Q

spectator ions

A

ions is in smale form in both sides of chem reaction , no change

27
Q

Acid + Alkaline

A

Produce water and salt

both neutralize each other

28
Q

system, surrounding, and universe

A

System: part of the universe of specific interest
(system is the substances involved
in a chemical or physical change)

Surroundings: the rest of the universe

Universe = System + Surroundings

29
Q

Thermochemistry

A

study of heat in chem reactions

30
Q

Thermla energy

A

energy associated with the random
motion of atoms and molecules

31
Q

Temp

A

how hot/cold something is
C* or K
Avg kenetic energy

32
Q

Heat

A

Transfer of thermal energy
J, cal, Cal (nutrition)
heat is absorbed or released during process

33
Q

thermodynamics

A

the study of the interconversion of heat and other kinds of energy

34
Q

system

A

the substances involved in a chemical or physical change
(the reactants and products)

defined as the substances involved in a chemical or
physical change

EX: H2O(s) –> H2O(l)
system ; ice, liquid water
surroundings: everything else

EX: reactants occuring in soluton

system: reactants and products

Surroundings: everything else , solvent (water)

35
Q

state functions

A

properties that are determined by the state of the system,
regardless of how that condition was achieved

36
Q

Internal energy (U)

A

sum of all kinetic & potential energy

ΔU is the change in the internal energy

37
Q

q=smΔT

A

q= heat
s= specific heat (ex. .240 j/g)
m= mass
ΔT= change in temp (75-20=55)

EX: (250g)(,240)(55)

38
Q

ΔU = q+ w

A

q= heat
w= work
(work is + when done on syatem, - when done by system)

EX:
Heat absorbed by the system (endothermic process)

q is positive

Heat released by the system (exothermic process)

q is negative

Work done on the system by the surroundings (e.g., a volume decrease)

w is positive

Work done by the system on the surroundings (e.g., a volume increase)
Ex: producing a gas, which expands

w is negative

The internal energy of a system can decrease (ΔU < 0) if it loses heat (q < 0)
or if it does work on the surroundings (w < 0)
Heat and Work: signs

39
Q

net ionic equation

A

what changes into solid

(liquid to solid or solid to liquid)

40
Q

Hybridization with multiple bonds

A

single bond; 1 sigma bond
double bond: 1 sigma + 1 pi
tripple bond: 1 sigma + 2 pi

41
Q

sigma bond

A

Direct, end-to-end overlap of orbitals in axis between nuclei

42
Q

pi bond

A

Sideways overlap of unhybridized p orbitals

43
Q

greenhouse gas

A

IR active

NOT a greenhouse gass :
O2 cause its homo diatomic = not IRactive

44
Q

electrolytes

A

strong acids / bases

has ions (neg and pos charge)

45
Q

covalent bond

A

covalent = non metal + non metal

46
Q

ΔT

A

energy/ (specific heat)(mass)

47
Q

need more solute than solvent in solution

A

solution

48
Q

A pi bond is formed by the…

A

side-by-side overlap of unhybridized p orbitals

49
Q

Which of the following statements about greenhouse gases is false

A

Ar, O2, and N2 are greenhouse gases because they have London dispersion forces

50
Q

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

A

combustion of fossil fuels

51
Q

A reaction gives off heat and produces a gas. What is the sign of the ∆H of this reaction?

A

neg

52
Q

Which of the following processes has contributed the most to the increasing atmospheric CO 2
concentration in recent years?

A

combustion of fossil fuels

53
Q

Why are H 2 O and CO 2 greenhouse gases, but N 2 and O 2 are not

A

H 2 O and CO 2 can undergo asymmetrical molecular vibrations by absorbing IR radiation,
whereas N 2 and O 2 cannot

54
Q

Fill in the blanks. Burning wood _________ heat; this is an ________ process

A

releases
exothermic

55
Q

When studying the thermochemistry of a particular reaction, we define the system as

A

the reactants and products of the reaction

56
Q

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

A

side-by-side
unhybridized p

57
Q

An exothermic reaction causes the surroundings to

A

warm up

58
Q

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

A

CO2 and CH4
IR

59
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

60
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

Both A and B are true

Chem (11 decks)

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