Quarterly Review (up to ch. 10)

Question 1

(ch 1) extensive properties relate to

Answer 1

how much matter is present in a sample

Question 2

(ch 1) intensive properties are characteristic of

Answer 2

the type of matter

Question 3

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

Answer 3

the same elements in the same proportions

Question 4

(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

Answer 4

ratio of small whole numbers

Question 5

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

Answer 5

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

Question 6

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

Answer 6

an acid and a base

Question 7

(ch 3) combustion reaction: involve reactions with

Answer 7

oxygen

Question 8

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

Answer 8

strong electrolytes

Question 9

(ch 4) molarity: the number of

Answer 9

moles of solute per liter of solution

Question 10

(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

Answer 10

equivalence point

Question 11

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

Answer 11

adding a measured amount of a second substance

Question 12

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

Answer 12

precipitated selectively

Question 13

(ch 5) heat transfers from … to …

Answer 13

warmer object; cooler object

Question 14

(ch 5) universe=

Answer 14

system + surroundings

Question 15

(ch 5) total energy =

Answer 15

KE + PE

Question 16

(ch 5) potential energy: energy of

Answer 16

condition or position

Question 17

(ch 5) enthalpy … be measured

Answer 17

cannot

Question 18

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

Answer 18

present conditions of the system

Question 19

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

Answer 19

1 K

Question 20

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

Answer 20

1 g sample by 1 K

Question 21

(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

Answer 21

enthalpy changes of the equations that were added

Question 22

(ch 4) soluble ionic compounds without exceptions:

Answer 22

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

Question 23

(ch 4) soluble ionic compounds with exceptions

Answer 23

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

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

Question 24

(ch 4) insoluble ionic compounds:

Answer 24

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

Question 25

(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

Answer 25

small; constant; random

Question 26

(ch 6) kinetic molecular theory: | gas particles are very small compared with

Answer 26

sample volumes

Question 27

(ch 6) kinetic molecular theory: | collisions of gas particles with each other and with the walls of the container are

Answer 27

elastic

Question 28

(ch 6) kinetic molecular theory: | the average kinetic energy of the gas particles is proportional to the

Answer 28

temperature on the kelvin scale

Question 29

(ch 6) kinetic molecular theory: | the gas particles do not all move at the same speed but have speeds given by the

Answer 29

maxwell-boltzmann distribution

Question 30

(ch 6) kinetic molecular theory: | exceptions to the premises of the theory occur at

Answer 30

high pressures and low temps

Question 31

(ch 6) 1 atm = ... torr

Answer 31

760

Question 32

(ch 6) 1 atm= ...kPa

Answer 32

101.325 kPa

Question 33

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

Answer 33

average kinetic energy; given temperature

Question 34

(ch 7) shorter wavelengths are

Answer 34

higher in energy

Question 35

(ch 7) order of visible light

Answer 35

VIBGYOR

Question 36

(ch 7) λ= (de Broglie)

Answer 36

h/mv

Question 37

(ch 7) distribution of wavelengths changes with

Answer 37

temperature

Question 38

(ch 7) greater value of n=

Answer 38

greater distance from nucleus

Question 39

(ch 7) l values are

Answer 39

0 to n-1

Question 40

(ch 7) ml values are

Answer 40

-l to l

Question 41

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

Answer 41

same set of four quantum numbers

Question 42

(ch 7) aufbau principle: electrons go into

Answer 42

lowest available energy level

Question 43

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

Answer 43

one electron in each orbital of the set

Question 44

(ch 8) isoelectronic series: same number of

Answer 44

electrons for group atoms and ions

Question 45

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

Answer 45

effective nuclear charge

Question 46

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

Answer 46

electron shielding→expanded radius

Question 47

(ch 8) ionization energy: energy required to

Answer 47

remove 1+ electrons

Question 48

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

Answer 48

most protons in the nucleus

Question 49

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

Answer 49

addition of an electron to a gaseous atom/ion

Question 50

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

Answer 50

exothermic (favorable)

Question 51

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

Answer 51

corresponding ions

Question 52

(ch 9) coulomb's law:

Answer 52

E= kQ1Q2/r

Question 53

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

Answer 53

shorter; stronger

Question 54

(ch 9) bond order=

Answer 54

bonds/ # regions of bonding

Question 55

(ch 9) dipole moment: measure of the

Answer 55

unequal sharing of electrons

Question 56

(ch 9) bond energy: energy required to break

Answer 56

1 mol of bonds in a gaseous species

Question 57

(ch 9) bond energies are

Answer 57

averages

Question 58

(ch 9) born-haber cycle:

Answer 58

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