Unit 1

Question 1

What is an element

Answer 1

consist of only one kind of atom, cannot be broken down

Question 2

What is a compound

Answer 2

two or more elements chemically bonded together into molecules/extended structures

Question 3

Daltons law of conservation of mass

Answer 3

total mass remains constant in a reaction

Question 4

Daltons law of constant (definite) composition

Answer 4

all samples of a given compound consist of the same mass fraction

Question 5

daltons law of multiple proportions

Answer 5

In different compounds of the same elements, the mass of combining the elements can be expressed in simple whole ratios

Question 6

Who discovered the existence of negatively charged particles (electrons)

Answer 6

Thomson; also made plum-pudding model

Question 7

Who did the oil drop experiment

Answer 7

Millikan

Question 8

What is Rutherford’s Scattering Experiment

Answer 8

Metal foil shot by alpha particles, where some got deflected backward by a positive charge (nucleus)

Question 9

The 3 subatomic particles

Answer 9

proton, neutron, electron

Question 10

what does Z stand for in atomic notation

Answer 10

Atomic number (protons)

Question 11

what does a stand for in atomic notation

Answer 11

mass number (protons + neutrons)

Question 12

What is an isotope

Answer 12

The same number of protons (Z) but differ in mass number (A)

Question 13

What group are the alkali metals

Answer 13

group 1, except H

Question 14

What group are the alkaline earth metals

Answer 14

group 2

Question 15

cation

Answer 15

positive ion, electron removed

Question 16

anion

Answer 16

negative ion, electron added

Question 17

what is a binary acid

Answer 17

contains no oxygen. hydro___ic acid

Question 18

name this acid: HCN (aq)

Answer 18

hydrocyanic acid

Question 19

Name this acid: HF (aq)

Answer 19

hydrofluoric acid

Question 20

name this acid: H2S

Answer 20

hydrosulfuric acid

Question 21

what is an oxyacid

Answer 21

contains H+O+nonmetal. name depends on the oxoanion

Question 22

What is the oxyacid name when oxoanion is hypo___ite

Answer 22

hypo___ous acid

Question 23

what is the oxyacid name when oxoanion is ___ite

Answer 23

___ous acid

Question 24

what is the oxyacid name when oxoanion is ___ate

Answer 24

___ic acid

Question 25

what is the oxyacid name when oxoanion is per__ate

Answer 25

per___ic acid

Question 26

absorption

Answer 26

excitation from a lower allowed energy level to a higher allowed energy level

Question 27

emission

Answer 27

relaxation from a higher allowed energy level to a lower allowed energy level (often ground level)

Question 28

what is a ground state

Answer 28

the electron is in the first orbit (n=1)

Question 29

what is ionization energy

Answer 29

The energy needed to completely remove the electron from the nucleus (n=infinity)

Question 30

Is energy positive or negative in absorption

Answer 30

positive

Question 31

Is energy positive or negative in emission

Answer 31

negative

Question 32

Is energy positive or negative in ionization

Answer 32

positive

Question 33

Infrared series (infrared radiation)

Answer 33

when electrons drop from outer orbits (n=4/5) to n=3

Question 34

visible series (visible radiation)

Answer 34

when electrons drop to n=2 orbit (first excited state)

Question 35

ultraviolet series (UV radiation)

Answer 35

when electrons drop to the n=1 orbit (ground state)

Question 36

how are energy and wavelength related

Answer 36

inversely; smallest energy is longest wavelength

Question 37

how are a photon's momentum and wavelength related

Answer 37

as momentum decreases, wavelength increases

Question 38

probability contour

Answer 38

the shape that defined the volume around the nucleus where the electron spends most of it's time

Question 39

how to calculate the number of radial nodes

Answer 39

n-l-1

Question 40

what is the n quantum number in each orbital

Answer 40

``` row of periodic table, starting at: s=1 p=1 d=3 f=4 ```

Question 41

what is the l quantum number in each orbital

Answer 41

s=0 p=1 d=2 f=3

Question 42

what is the ml quantum number

Answer 42

s=0 p= -1 to +1 d= -2 to +2 f= -3 to +3

Question 43

what shape is the s orbital

Answer 43

big sphere

Question 44

what shape is the p orbital

Answer 44

dumbbell shape

Question 45

what shape is the d orbital

Answer 45

clover type thing, nodal planes lie between the orbital lobes

Question 46

how to find number of angular nodes

Answer 46

given by l

Question 47

how to find total number of nodes

Answer 47

n-1

Question 48

Pauli's Exclusion Principle

Answer 48

no two electrons can have all four quantum numbers alike

Question 49

What is Zeff

Answer 49

an effective nuclear charge (the nuclear charge and electron actually experiences due to shielding electrons

Question 50

Greater nuclear charge ___ orbital energy

Answer 50

lowers

Question 51

electron-electron repulsion _____ orbital energy

Answer 51

raises

Question 52

electrons in higher n are shielded from the full nuclear charge so they have ___ energy

Answer 52

higher

Question 53

orbitals with good penetration have ____ energy

Answer 53

lower

Question 54

order the orbitals from least shielding/penetration to most shielding/penetration

Answer 54

f,d,p,s

Question 55

order the orbitals in order from lowest energy to highest energy

Answer 55

s,p,d,f

Question 56

Hunds rule

Answer 56

when there are orbitals of equal energy, maximize unpaired spins first before doubling up

Question 57

Cr and Cu have what

Answer 57

anomalous configurations, attributed to special stability of 3d subshells (doesn't follow the normal way fo writing quantum) Also includes Cr, Cu, Mo, Ag, Au

Question 58

How do transition metals lose electrons to form cations

Answer 58

s electrons are removed before the d electrons since d has a much lower energy

Question 59

paramagnetic

Answer 59

unpaired electrons

Question 60

diamagnetic

Answer 60

all electrons paired

Question 61

Compare the sizes of Li and Li+

Answer 61

cations smaller than atoms Zeff increases as there is a net positive charge Radius decreases

Question 62

Compare the sizes of F and F-

Answer 62

anions are larger than atoms Zeff decreases as there is a net negative charge radius increases

Question 63

What is the periodic trend of ionic size

Answer 63

down a group: ionic size increases | across a period: anion size decreases with decreasing charge (number not actual value)

Question 64

rank in order of increasing ionic size: | K+, S2-, Cl-

Answer 64

K+ < Cl- < S2-

Question 65

metallic radius

Answer 65

one half the shortest distance between nuclei of bonded atoms

Question 66

covalent radius

Answer 66

one half shortest distance between nuclei of adjacent individual atoms

Question 67

How does Zeff relate to atomic size

Answer 67

As Zeff increases atomic size decreases

Question 68

What is the periodic trend of atomic radius

Answer 68

across a period and up a period atomic radius decreases (biggest in bottom left, smallest in top right)

Question 69

What is the periodic trend of ionization energy

Answer 69

opposite of atomic radius, (biggest in top right, smallest in bottom left) (anomaly between N and O, and Be and B)

Question 70

what is the periodic trend of electron affinity

Answer 70

increases across a period and decreases down a group

Question 71

What are the 4 periodic trends about bonding

Answer 71

Zeff, IE, EA all increase up and across, while atomic radius is opposite

Question 72

What is the periodic trend of metallic behavior

Answer 72

metallic behavior decreases up and across

Question 73

what is the group 1 periodic trend of reactivity, and what agent is it

Answer 73

reactivity increases down group 1, good reducing agent

Question 74

What is the period trend of halogen reactivity, and what agent is it

Answer 74

halogen reactivity decreases down the group, good oxidizing agent