Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

AP Chemistry > Quarterly Review (up to ch. 10) > Flashcards

Quarterly Review (up to ch. 10) Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

(ch 1) extensive properties relate to

A

how much matter is present in a sample

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

(ch 1) intensive properties are characteristic of

A

the type of matter

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

(ch 2) law of constant composition: all samples of a pure substance contain

A

the same elements in the same proportions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

(ch 2) law of multiple proportions: for different compounds formed from the same elements, the masses of one element that combine with a fixed mass of the other are in a

A

ratio of small whole numbers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

(ch 2) atomic mass unit (u) is defined as exactly

A

1/12 off the mass of a carbon-12 atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

(ch 3) neutralization reaction: chemical reaction that takes place between

A

an acid and a base

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

(ch 3) combustion reaction: involve reactions with

A

oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

(ch 4) most ionic compounds and a few molecular compounds dissociate completely into ions in water and are known as

A

strong electrolytes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

(ch 4) molarity: the number of

A

moles of solute per liter of solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

(ch 4) indicators that change color at or near the .. are used to determine when an equivalent amount of the solution of known concentration has been added

A

equivalence point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

(ch 4) titration: a procedure to determine the quantity of one substance by

A

adding a measured amount of a second substance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

(ch 4) gravimetric analysis: one component of a solution is …., separated from solution, dried, and weighed

A

precipitated selectively

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

(ch 5) heat transfers from … to …

A

warmer object; cooler object

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

(ch 5) universe=

A

system + surroundings

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

(ch 5) total energy =

A

KE + PE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

(ch 5) potential energy: energy of

A

condition or position

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

(ch 5) enthalpy … be measured

A

cannot

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

(ch 5) state function: any property of a system that is determined by the

A

present conditions of the system

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

(ch 5) heat capacity: the quantity of heat required to increase the temperature of that object by

A

1 K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

(ch 5) specific heat: heat needed to increase the temp of a

A

1 g sample by 1 K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

(ch 5) hess’s law states that the change in enthalpy for an equation obtained by adding two or more thermochemical equations is the sum of the

A

enthalpy changes of the equations that were added

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

(ch 4) soluble ionic compounds without exceptions:

A

group 1 metals, NH4+, nitrates, perchlorates, acetates

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

(ch 4) soluble ionic compounds with exceptions

A

chlorides, bromides, iodides (except: ag+, Hg2^2-, Pb2+)

sulfates (hg2^2-, Pb2+, Sr2+, Ba2+)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

(ch 4) insoluble ionic compounds:

A

carbonates (ex. group 1, nh4+)
phosphates (ex. group 1, nh4+)
hydroxides (ex. group 1, NH4+, Sr2+, Ba2+)

25
Q

(ch 6) kinetic molecular theory:
gases are .. particles in … and … motion, and there are no forces of attraction or repulsion between any 2 gas particles

A

small; constant; random

26
Q

(ch 6) kinetic molecular theory:

gas particles are very small compared with

A

sample volumes

27
Q

(ch 6) kinetic molecular theory:

collisions of gas particles with each other and with the walls of the container are

A

elastic

28
Q

(ch 6) kinetic molecular theory:

the average kinetic energy of the gas particles is proportional to the

A

temperature on the kelvin scale

29
Q

(ch 6) kinetic molecular theory:

the gas particles do not all move at the same speed but have speeds given by the

A

maxwell-boltzmann distribution

30
Q

(ch 6) kinetic molecular theory:

exceptions to the premises of the theory occur at

A

high pressures and low temps

31
Q

(ch 6) 1 atm = … torr

A

760

32
Q

(ch 6) 1 atm= …kPa

A

101.325 kPa

33
Q

(ch 6) all gases have the same …. at a ….

A

average kinetic energy; given temperature

34
Q

(ch 7) shorter wavelengths are

A

higher in energy

35
Q

(ch 7) order of visible light

A

VIBGYOR

36
Q

(ch 7) λ= (de Broglie)

A

h/mv

37
Q

(ch 7) distribution of wavelengths changes with

A

temperature

38
Q

(ch 7) greater value of n=

A

greater distance from nucleus

39
Q

(ch 7) l values are

A

0 to n-1

40
Q

(ch 7) ml values are

A

-l to l

41
Q

(ch 7) pauli exclusion principle: no two atoms can have the

A

same set of four quantum numbers

42
Q

(ch 7) aufbau principle: electrons go into

A

lowest available energy level

43
Q

(ch 7) hund’s rule: electrons in degenerate orbitals do not pair until there is

A

one electron in each orbital of the set

44
Q

(ch 8) isoelectronic series: same number of

A

electrons for group atoms and ions

45
Q

(ch 8) atomic radii decrease across periods due to increase in

A

effective nuclear charge

46
Q

(ch 8) atomic radii increase down groups due to increased

A

electron shielding→expanded radius

47
Q

(ch 8) ionization energy: energy required to

A

remove 1+ electrons

48
Q

(ch 8) in an isoelectronic series, the ionization energy is greatest for the species with the

A

most protons in the nucleus

49
Q

(ch 8) electron affinity: energy change that accompanies the

A

addition of an electron to a gaseous atom/ion

50
Q

(ch 8) in general, elements to the right side and at the top of the periodic table have … elecron affnities

A

exothermic (favorable)

51
Q

(ch 9) lattice energy: energy required to separate one mole of crystal lattice into

A

corresponding ions

52
Q

(ch 9) coulomb’s law:

A

E= kQ1Q2/r

53
Q

(ch 9) the higher the bond order, the … and … the bond

A

shorter; stronger

54
Q

(ch 9) bond order=

A

bonds/ # regions of bonding

55
Q

(ch 9) dipole moment: measure of the

A

unequal sharing of electrons

56
Q

(ch 9) bond energy: energy required to break

A

1 mol of bonds in a gaseous species

57
Q

(ch 9) bond energies are

A

averages

58
Q

(ch 9) born-haber cycle:

A

5 simpler reactions; most reactions don’t occur in one step

AP Chemistry (24 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions