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88 Terms

1

Element

cannot be made simpler, building block of matter. Includes diatomics, atoms, and even polyatomic

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2

Compound

Pure substances that can be broken down by chemical means ie. NaCl

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3

Atoms

Neutral particles

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4

molecules

Smallest physical unit, always neutral eg. a molecule of H2O

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5

elements of a chemical formula

subscripts (number of atoms), superscript (charge), coefficient (# compounds), balanced

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6

accurate

results close to the actual number

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7

precise

results close to each other

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8

Physical properties

appearance, smell, feel, melting point, density, etc

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9

chemical properties

how things react ex. Mg burns in air

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10

wtf is a barometer or a manometer

google it bitch

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11

Methods of separation

decanting, filtration, distillation, evaporation

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12

diatomics

H O N F I Cl Br

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13

Ammonium

NH4 +

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14

Hydroxide

OH -

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15

Nitrate

NO3 -

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16

Sulfate

SO4 2-

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17

Carbonate

CO3 2-

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18

Phosphate

PO4 3-

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19

Diatomic tool

NICK the BABY CAMEL ate and INCH CLAM and CREPES for SUPPER in PHOENIX

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20

Practice naming

don’t procrastinate

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21

What is the number of protons

constant, atomic #

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22

How to find neutrons

Mass-Protons/atomic #

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23

Single replacement reaction

compound breaks apart and combines with the other reactant which is typically an element

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24

Double replacement reaction

Both reactants break apart and recombine into two new parts

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25

Synthesis/combination reaction

Several reactants combine to form a single product

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26

decomposition reaction

a compound breaks down bc of a chemical change

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27

Combustion reaction

tends to make H2O+CO2, reaction w/ O2 that produces light and heat

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28

Group I solubility

soluble

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29

NO3 - solubility

soluble

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30

NH4+

soluble

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31

Famous Precipitates

BaSO4 (white), PbI2 (bright yellow), AgCl, AgBr, AgI (white to pale yellow)

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32

Precipitate Reaction

AB + XY = XB + AY (two ionics make at least one non soluble product)

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33

Which are almost always (always when not with an always soluble) insoluble?

OH- (hydroxide), CO3 2- (carbonate), C2O4 2- (oxalate), PO4 3- (phosphate), "heavy metals"

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34

electron configuration

1s2 2s2 2p5 etc (in order spdf)

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35

What are orbital diagrams

the up down arrow ones

<p>the up down arrow ones</p>
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36

Coulomb's law

the force of attraction or repulsion between two charged particles is directly proportional to the product of the charges and inversely proportional to the distance between them. F = (kq1q2)/dˆ2

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37

As an electron moves away from the nucleus it's potential energy...

..increases

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38

what is special about transition metal ions?

they lose electrons from the s sublevel before d

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39

isometric

same electron configuration (K+, Cl-, S2-, Ar)

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40

periodic groups are...

...columns, # of electrons in outer shell

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41

periodic periods are...

...rows, # of shells

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42

transition element properties

conductive, malleable, for ions with variety of positive charges, act as good catalysts, often form colored compounds, form variety of alloys

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43

valence electrons

outermost electron ring (highest energy level)

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44

core electrons

\n all non valence electrons

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45

effective strength formula

proton # - # core electrons = strength of + on valence e-

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46

electronegativity/electron affinity

how much an element will attract electrons. increases (+ charge increases) across the periodic table, and decreases (greater atomic radii) descending

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47

ionization energy (IE)

energy required to remove an electron. increases across (+ charge increases) and decreases descending periodic table (more barriers)

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48

Evaporation is endothermic or exothermic

endothermic, need to GIVE it heat

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49

cation

positive, metal

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50

anion

negative, non-metal

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51

Order of IMFs (least to greatest)

Disperson, dipole-dipole, hydrogen

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52

Trigonal pyramidal

4 e- pairs, 3 bonds, 1 lone pair

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53

Tetrahedral

4 e- pairs, all bonds

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54

Octahedral

6 e- pairs, all bonds, x,y,z

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55

Trigonal planar

3 e- pairs, all bonds, flat

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56

Linear

2 e- pairs, all bonds, a line

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57

Bent

4 e- pairs, 2 bonds, 2 lone pairs, angle

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58

Water's normal boiling point is 100˚C, why can water evaporate at 20˚C?

Because of random velocities of water molecules causing some to have a high enough kinetic energy to escape from the surface.

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59

What havens to water vapor pressure in a container with ice melting at room temp?

Increases rapidly, then more slowly until reaching equilibrium

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60

What happens to the rate of condensation?

Increases until it equals the rate of evaporation and then remains constant.

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61

What are the affects of temp, IMFs, and molar mass on the vapor pressure of a substance?

Vapor pressure increases with an increase in temp and a decrease in strength of IMFs and molar mass.

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62

When, in general, does a liquid begin to boil?

\n When the vapor pressure equals the outside pressure

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63

Why does ice have a lower density than water>

than water>

Because of the crystal structure formed by hydrogen bonds and its open structure.

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64

hydrogen bonds occur when hydrogen is bonded to which elements

F, O, N

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65

kinetic molecular theory

gas molecules are in constant random motion, when they collide energy is not lost, do not attract each other, far apart, same temp, same average kinetic energy

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66

kinetic energy formula

KE=1/2mvˆ 2

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67

pressure and force formula

p=f/a

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68

Formula for pressure, volume, and temp

pv/t = pv/t

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69

Dalton's law of partial pressures

Since gas pressure depends on # of molecules not their mass or size, it is easy to see that each gas in a mixture contributes pressure according to the number of molecules present.

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70

Graham's Law

small particles diffuse faster

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71

˚ C to K

+273

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72

atm to mmHg

atm x 760

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73

How do gasses exert pressure?

Tiny molecules colliding with every pinhead-sized area of any surface. # of collisions is identical, forces add up for exert a force on the whole surface, creating a uniform "pressure".

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74

Which is larger: proportional more collisions or harder collisions

samsies

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75

mole to liter (for gasses)

1 mol = 22.4L

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76

molar mass

g/mol

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77

particles / mol

6.02x10ˆ 23

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78

Relative atomic mass

average atomic mass of all isotopes based on how common they are: (mass(%)+mass(%))/100

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79

percent composition by mass

mass/total mass

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80

density=

m/v

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81

molarity

mass of solute per solution: moles of solute/liters

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82

Dilution rule

concentration 1(volume 1) = concentration 2(volume 2)

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83

Ideal gas law

PV = nRT

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84

When will something produce a smell

when it is polar

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85

When something has a charge, the polarity is…

Not applicable

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86

manometer gas pressure shit

if gas is lower than outside: atmosphere pressure - height (mm) = gas pressure (mmHg)

If gas is greater than out side side: atmosphere pressure + height (mm) = gas pressure (mmHg)

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87

percent error

(|accepted-measured| x 100) / accepted

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88

is phase change a physical or chemical change

physical

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