Chm Terms Exam #2

Front 1

Stoichiometry

Back 1

-can be used to predict (calculate) amounts & products

Front 2

Limiting Reactant

Back 2

Reactant that is completely consumed before any other chemical in a reaction
-limits how much product can be made
-other reactants are NOT consumed fully (in excess)

Front 3

Theoretical Yield

Back 3

specific maximum of product that can be made

Front 4

Actual Yield

Back 4

What we make (less than theoretical)

Front 5

% yield=

Back 5

(actual yield/theoretical yield)x 100

Front 6

Solution (Define)

Back 6

homogenous mixture of 2 substances

*solute + solvent*

Front 7

Solute (Define)

Back 7

Stuff that is dissolved

-Minor componet

Front 8

Solvent (Define)

Back 8

Stuff that is doing the dissolving

-major component

Front 9

Concentration

Back 9

amount of solute in solution

Front 10

Molarity (M)=

Back 10

moles of solute ÷ volume of solution (L)

Front 11

Stock Solution (Define)

Back 11

way to store solution in lab

Front 12

Diluted Solutions`

Back 12

-less concentrated solution

-smaller molarity

-#moles does NOT change, only volume changes

Front 13

Diluted Solution Equation

Back 13

M₁V₁=M₂V₂

Front 14

Electrolyte

Back 14

material forms ions in solution & will conduct electricity

Front 15

Strong Electrolyte

Back 15

completely dissolves in water

Front 16

Weak Electrolyte

Back 16

dissociates, not completely

Front 17

How do you know if you have an electrolyte?

Back 17

-soluble ionic compounds (strong electrolyte)

-slightly soluble salts (weak electrolyte)

-molecular compounds (accept acid/base)= non-electrolytes, including pure elements

Front 18

Strong Acid

Back 18

ionizes (dissociates) completely in a solution

Ex: HCL(aq) →H⁺(aq) and Cl⁻(aq)

Front 19

Weak Acid

Back 19

ionizes (dissociates) a little bit

Ex: HC₂H₃O₂(aq) ↔ H⁺(aq) + C₂H₃O₂ (aq)

Front 20

In order for Ionic compounds to conduct electricity they must_____.

Back 20

dissolve (be soluble) in water

Front 21

Salt

Back 21

ionic compounds that result from the neutralization reaction of an acid and a base

Front 22

Aqueous + Aqueous = Aqueous + Aqueous

signifies____.

Back 22

There was NO REACTION

Front 23

Molecular Equation

Back 23

Complete neutral formulas

reactions + products

Front 24

Complete Ionic Equation

Back 24

-list all ions present in a reaction

Front 25

Spectator Ions

Back 25

aqueous ions that exist as both reactants & products

Front 26

Acid-Base Reaction

Back 26

Acid&Base neutralize eachother

Acid + Base → Water + Salt

Front 27

Polyprotic Acid

Back 27

can lose more than one H⁺ in a solution

Front 28

Titration

Back 28

method of following a reaction until is is stoichiometry complete

-reached end point (equivalence point)

-no excess

Front 29

Indicator (during experiment)

Back 29

determines endpoint of experiment (changes color when endpoint is reacher)

Front 30

Gas-Evolution Reactions

(list 4)

Back 30

1) Sulfides: product H₂S

2) Carbonates & bicarbonates: product CO₂

3) Sulfites & bisulfites: product SO₂

4) Ammonium: product NH₃

Front 31

Redox Reactions

Back 31

Transfer of electrons from one atom to another

-often involves O₂(g)

Front 32

Oxidation

Back 32

loss of electrons (more positive)

Front 33

Reduction

Back 33

gain of electrons (more negative)

Front 34

Free elements are assigned an oxidation state of __.

Back 34

zero

Cu, Le, Si, H₂, N₂, O₂, F₂, Cl₂, P₄, etc.

Front 35

Any simple monatomic anion is assigned an oxidation state____.

Back 35

equal to it's charge

Front 36

Alkali Metals (Group 1A) in ionic compounds are assigned an oxidation state of ____.

Back 36

+1

Front 37

Fluorine in compounds is ALWAYS assigned an oxidation state of ____.

Back 37

-1

Front 38

Alkaline Earth Metals (IIA) in compounds are always assigned a ____ oxidation state.

Back 38

+2

Front 39

Zn & Cd in compounds are always assigned a ____ oxidation state.

Back 39

+2

Front 40

Al & Ga in compounds are always assigned a ____ oxidation state.

Back 40

+3

Front 41

Hydrogen bound to a non-metal is assigned a ___ oxidation state.

Back 41

+1

Front 42

Hydrogen bound to a metal is assigned a ____ oxidation state.

Back 42

-1

Front 43

Oxygen in compounds is assigned a ____oxidation state, except in peroxide where it's assigned ____.

Back 43

oxygen in compounds = -2

O₂=-1

Front 44

The sum of the oxidation states of all atoms in a species must be equal to the _____.

Back 44

net charge

Front 45

Activity Series (define)

Back 45

ability of a metal to be oxidized

-Top: most easily oxidized (best deducting agents)

-Bottom: best oxidizing agents (noble metals)

Front 46

Metal ABOVE ion →

Back 46

reaction occurs

Front 47

Metal BELOW ion

Back 47

no reaction occurs

Front 48

Electrons Mass=

Back 48

one trillionth of one trillionth of a gram

Front 49

Electrons determines atoms ____ & ____. Ions & Bonding.

Back 49

physical & chemical properties

Front 50

Spectroscopy

Back 50

shine light on stuff and see how it reacts

Front 51

Wave-Particle Duality

Back 51

light behaves as both a wave and a particle

Front 52

Why do we study light?

Back 52

It's very similar to the electron

Front 53

Light (define)

Back 53

electromagnetic radiation

-has a wavelength & frequency

Front 54

Electric Field

Back 54

electrically charged particles that can experience a force

Front 55

Magnetic Force

Back 55

magnetic particle that experiences force

Front 56

Electromagnetic Waves travel at a____ speed.

Back 56

travel at a CONSTANT speed.

Front 57

Amplitude (define)

Back 57

height of wave

-determines brightness/intensity of light

Front 58

Wavelength (symbol, units, equation, define)

Back 58

λ

meters (m)

λ=c÷V

distance between 2 PEAKS in a wave

Front 59

Frequency (symbol, units, equation, define)

Back 59

V

Hz (S⁻¹)

V=c÷λ

number of waves that pass a point in a given period of time

Front 60

Color is determined by ____.

Back 60

wavelength or frequency

Front 61

White Light is ____.

Back 61

a mixture of all colors

Front 62

Color of an object is the reflected light that the object ______.

Back 62

did not absorb

Front 63

Short Wave Length

Back 63

hight frequency=high energy (gamma rays)

Front 64

Long Wave Length

Back 64

low frequency=low energy

Front 65

Light behaves light waves except for ____. (list the 3 exceptions)

Back 65

1) Black Body Radiation (Thermal Radiation)

2) Photoelectric Effect

3) Atomic Spectroscopy

Front 66

Black Box Radiation (Thermal Radiation)

Back 66

Hot objects emit radiation in a specfic spectrum of frequencies & intensities, VARYING with TEMP of object.

Front 67

Hotter Object= ___wavelengths.

Back 67

shorter wavelengths

blue (blue-white flame)

Front 68

Cooler Objects=____wavelengths.

Back 68

longer wavelengths

red (toaster)

Front 69

Plank proposed____.

Back 69

Light is delivered in packets (quanta)

---> PHOTONS (behave as tiny particles)

Front 70

Photoelectric Effect

Back 70

Shining Light on a metal surface → electrons fly off

Front 71

Eistein discovered the _____ exception.

Back 71

Photoelectric Effect

Front 72

Threshold Frequency

Back 72

Wavelength & Frequency are needed to emit electrons regardless of intensity of light (brightness)

Front 73

Atomic Spectrum

Back 73

When an atom absorbs energy, that energy is often released as light energy

-each element (gas state) has it's own characteristic line spectrum

Front 74

White Light→Prism→Rainbow (_____)

Back 74

continuous spectrum

Front 75

Light from atom→Grating→emission (____)

Back 75

line

Front 76

Heinsenberg Uncertainty Principle

Back 76

-Wave and Particle Nature are complimentary properties

(more you know about one, less you know about other)

-Product of uncertainty in both position and speed of a particle are inversely proportioned to mass

Front 77

Schrödiner

Back 77

Wave-Particle Duality

Hγ=Eγ

Front 78

Bohr predicted____.

Back 78

electrons travel around nucleus in orbits

-electrons exist only at FIXED distances from nucleus

-energy of orbits are FIXED →Stationary States

Front 79

∆=negative, electron moves _____ to nucleus. Photon is _____.

Back 79

electron moves CLOSER to nucleus.

photon is EMITTED.

Front 80

∆=positive, electron moves____to nucleus.

Photon is___.

Back 80

electron moves FARTHER from nucleus.

Photon is ABSORBED.

Front 81

Principle Quantum Number (symbol, define)

Back 81

n

-size & energy of an orbital

as n increase, orbital gets bigger

(electrons are further from nucleus)

n≥l (integer; n=1,2,3,…)

n=principle level

Front 82

Angular Momentum Quantum (symbol, define)

Back 82

L (lowercase)

-shape of orbital where electron resides

L = 0,1,2,3…n-1 (always less than n)

(L= possible sublevels) = # values of L

Front 83

L = 0 →

Back 83

s

Front 84

L = 1→

Back 84

p

Front 85

L = 2 →

Back 85

d

Front 86

L = 3 →

Back 86

f

Front 87

Magnetic Quantum Number (symbol, define)

Back 87

m

orientation of orbital

mι=-L,…-2,-1, 0, 1, 2, …, +L

Front 88

S Orbital (L=__, define, shape)

Back 88

L=0

each principle energy level has an S-orbital

LOWEST shell

-spherical shape

Front 89

P Orbital (L=___, define, shape)

Back 89

L=1

orientation is different

→P×, Ps, Pz

-2 lobes (Bowtie)

Front 90

d Orbital (L=___, define, shape)

Back 90

L=2

4 planes

dxy, dxz, dyz, dx²-y², dz²

-clover leaf shape

Front 91

f Orbital (L=___)

Back 91

L=3