CHM 2045 - Final

Question 1

Most of the volume of an atom is empty space, throughout which are dispersed _________.

Answer 1

electrons

Question 2

Cathode ray tubes were used in the discovery of ________.

Answer 2

electrons

Question 3

The law of conservation of mass states that in a chemical reaction, matter is never ….?

Answer 3

created nor destroyed

Question 4

Most of an atom’s mass and all of its positive charge are contained in the atom’s _______.

Answer 4

nucleus

Question 5

Nonmetals tend to gain electrons to form _______.

Answer 5

anions

Question 6

The number of ______ in an atom defines its identity.

Answer 6

protons

Question 7

The percentage of a particular isotope of an atom found in a natural sample of that element is called the _______ ________.

Answer 7

natural abundance

Question 8

______ are good conductors of heat and electricity, often shiny, ductile, malleable, and tend to lose electrons when undergoing a chemical change.

Answer 8

Metals

Question 9

One of the postulates of John Dalton’s atomic theory is that each element is composed of tiny, indestructible particles called _____.

Answer 9

atoms

Question 10

______ are positively charged ions.

Answer 10

Cations

Question 11

Avogadro’s number is the number of atoms contained in exactly 12g of ______-__.

Answer 11

carbon-12

Question 12

The average mass of a molecule is the _______ _____.

Answer 12

formula mass

Question 13

A(n) ________ reaction is a reaction in which a substance combines with oxygen to form carbon dioxide.

Answer 13

combustion

Question 14

A(n) ______ bond typically occurs between a metal and a non-metal.

Answer 14

ionic

Question 15

The _______ formula gives the number of atoms of each element in a molecule of a compound.

Answer 15

molecular

Question 16

_______ compounds are compounds that contain only two elements.

Answer 16

Binary

Question 17

The _____ _______ composition of an element is that element’s percentage of a compound’s total mass.

Answer 17

mass percent

Question 18

A(n) _______ bond occurs between two non-metals.

Answer 18

covalent

Question 19

Many molecular elements exist as ________ molecules.

Answer 19

diatomic

Question 20

Organic compounds that contain only carbon and hydrogen are called __________.

Answer 20

hydrocarbons

Question 21

The species that limits the amount of product that is formed in a chemical reaction is the ________ _______.

Answer 21

limiting reactant

Question 22

______ reactions are those in which electrons are transferred from one species to another.

Answer 22

Redox

Question 23

When a species is dissolved in water but does not form a solution that conducts electricity, it is called a(n) ___________.

Answer 23

nonelectrolyte

Question 24

The ______ _____ is a numerical measure of the relationship between the actual yield and the theoretical yield.

Answer 24

percent yield

Question 25

A reaction in which two solutions combine to form a solid is called a(n) ________ reaction.

Answer 25

precipitation

Question 26

The numerical relationships between chemical amounts in a balanced reaction are called reaction ___________.

Answer 26

stoichiometry

Question 27

The sum of oxidation states of all atoms in an ion is equal to the ____ charge.

Answer 27

ion

Question 28

________ ions are species that are not involved in the chemistry of a solution phase reaction.

Answer 28

Spectator

Question 29

A(n) _______ _________ is a species that dissociates completely in a solution to form ions.

Answer 29

strong electrolyte

Question 30

Dalton's law of _______ ______ states that the total pressure of a gas sample is equal to the sum of the partial pressures of its components

Answer 30

partial pressures

Question 31

The average distance that a particle can travel in between collisions is called its _____-____-____.

Answer 31

mean-free-path

Question 32

The average kinetic energy of a particle is proportional to its _________ in units of ______.

Answer 32

temperature, Kelvin

Question 33

_______ is the force exerted per unit area by gas particles as they strike the walls of a container.

Answer 33

Pressure

Question 34

Pressure and volume are ________ proportional.

Answer 34

inversely

Question 35

A mercury barometer is a device that measures pressure in units of _____.

Answer 35

mmHg

Question 36

The molar volume of an ideal gas at STP is always ____ L

Answer 36

22.4

Question 37

How do you calculate mole fraction?

Answer 37

Xa = na/nTotal Xa = pa/pTotal

Question 38

How do you calculate partial pressure?

Answer 38

Pa = Xa(Ptotal)

Question 39

How do you calculate density?

Answer 39

D = P(MM)/RT

Question 40

The SI units of energy are the _____.

Answer 40

joule

Question 41

1 cal = _____ J

Answer 41

4.184

Question 42

1 KJ = _____ J

Answer 42

1000J

Question 43

A(n) _______ is defined as the amount of energy required to raise the temperature of 1g of water by exactly 1ºC.

Answer 43

calorie

Question 44

A ______ function is one that depends only on the initials and final values, but not on the manner in which the system was prepared.

Answer 44

state

Question 45

When heat is absorbed by a system, the sign of delta H is _______.

Answer 45

positive

Question 46

A positive value of work is obtained when work is done ___ the system.

Answer 46

on

Question 47

The measure of a substance's intrinsic capacity to absorb heat is called its _____ ________.

Answer 47

heat capacity

Question 48

When a closed system expands, the sign of work is ________.

Answer 48

negative

Question 49

An ________ reaction is one that absorbs heat from its surroundings.

Answer 49

endothermic

Question 50

The phenomenon of light bending around an obstacle or slit is called ________.

Answer 50

diffraction

Question 51

The ________ quantum number determines the orientation of an orbital

Answer 51

magnetic

Question 52

Delta E = __ + __

Answer 52

Detla E = q + v

Question 53

q = __ x __ x __

Answer 53

q = m x cs x detla T

Question 54

w = -__ x __

Answer 54

w = -p x delta V

Question 55

1 L x atm = _____ ?

Answer 55

101.3 J

Question 56

qrxn = - ( __ x __ x __ )

Answer 56

qrxn = - (m x cs x delta T)

Question 57

Delta Hrxn = ____/____

Answer 57

Delta Hrxn = qrxn/mole

Question 58

_________ radiation is a type of energy embodied in oscillating electric and magnetic fields.

Answer 58

Electromagnetic

Question 59

A _____ is a point where the wave function goes through zero.

Answer 59

node

Question 60

The highest energy region of the electromagnetic spectrum is _____ ______.

Answer 60

gamma rays

Question 61

__________ _______ occurs when two waves travel in phase with on another.

Answer 61

Constructive interference

Question 62

Energy is _______ from an atom when an electron moves to a lower energy level.

Answer 62

emitted

Question 63

The ________ uncertainty principle relates the uncertainty in an electron's position to the uncertainty in its velocity.

Answer 63

Heisenberg

Question 64

The more certainly you know a given property, the less certain you know its __________ property.

Answer 64

complementary

Question 65

Which quantum number determines the overall size and approximate energy of an orbital?

Answer 65

Principal quantum number

Question 66

Which quantum number primarily determines the shape of the orbital?

Answer 66

Angular momentum quantum number

Question 67

The __________ ______ is the observation that many metals emit electrons when light is shined upon them.

Answer 67

photoelectric effect

Question 68

v = __/__

Answer 68

v = c/lamda

Question 69

1m = 1^ ? nm?

Answer 69

1m = 1^9 nm

Question 70

h = _______ (Plank's constant)

Answer 70

6.626x10^-34 J/s

Question 71

E = __ x __

Answer 71

E = hv

Question 72

E could also equal....?

Answer 72

E = hc/lamda

Question 73

E photon = _____/______

Answer 73

E photon = E total/# photons

Question 74

photon's = ______/______

Answer 74

photons = E pulse/E photon

Question 75

De Broglie Wavelength Lamda = __/__ x __

Answer 75

Lamda = h/mv *the mass must be in kg

Question 76

Excited electron...from low "n" to high "n" ______ a photon.

Answer 76

absorbs

Question 77

Relaxed electron...from high "n" to low "n" ______ a photon.

Answer 77

emits

Question 78

Wavelength is _______ proportional to frequency.

Answer 78

inversely

Question 79

The lowest energy state of an atom is its ______ ______.

Answer 79

ground state

Question 80

_______ are charged species that are much smaller than their corresponding atoms.

Answer 80

Cations

Question 81

An element with unpaired electrons is considered ___________.

Answer 81

paramagnetic

Question 82

The effective nuclear charge differs from the actual nuclear charge due to ________.

Answer 82

shielding

Question 83

______ ________ principle: Implies that each orbital can have a maximum of only two electrons , with opposing spins.

Answer 83

Pauli Exclusion

Question 84

_____ ______: When filling degenerate orbitals, electrons fill them singly first, with parallel spins.

Answer 84

Hund's Rule

Question 85

The _________ energy is the energy required to remove an electron from an atom or ion in the gaseous state.

Answer 85

ionization

Question 86

Degenerate orbitals have the same ______.

Answer 86

energy

Question 87

The ability of an atom of attract electrons to itself in a chemical bond is called ___________.

Answer 87

electronegativity

Question 88

The ______ ______ of an atom is the charge it would have if all the bonding electrons were shared equally between the atoms.

Answer 88

formal charge

Question 89

How do you calculate formal charge?

Answer 89

F.c = ve - lone pairs - 1/2(bonding pairs)

Question 90

Expanded octets occur for elements in the ______ row or below.

Answer 90

third

Question 91

The lattice energy ________ when the size of the cation increases.

Answer 91

decreases