Unit 1 Test

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39 Terms

1

Solution

solute dissolved in solvent

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2

Salt dissolved in water

Attraction between water + sodium and water + chloride is stronger than sodium + chloride

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3

Endothermic

Separates molecules

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4

Exothermic

Joins molecules

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5

Why do solids conduct

Ion movement → ion collisions that carry charge

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6

Level of conductivity

Determined by number of ions and collisions

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7

Iodine in water

Iodine’s temporary dipole forms induced dipole bond with water

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8

Iodine in water hexane added

Hexane and iodine more attracted to each other

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9

Why do particles form solids

Kinetic energy and temperature

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10

Ionic solids

Electrostatic attraction

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11

Molecular solids

LDF, dipole-dipole, H-bonds

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12

Metallic solids

Positive ions surrounded by a sea of electrons, metallic bond

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13

Covalent network

Covalent bonds

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14

Graphite

Conducts in horizontal planes and is a lubricant

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15

Acid

Proton donor

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16

Base

Proton acceptor

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17

Ph scale

Increment in one pH is 10x H+/OH-

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18

Strong acids

H2SO4, HI, HBr, HNO3, NCl, HClO4

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19

Strong bases

First two columns on table

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20

Neutralization

Acid and base react to form a salt and water, moles H+ = moles OH-

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21

Incomplete neutralization

Moles of H+ or OH- left over

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22

Oxidation

Electron removed

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23

Reduction

Electron added

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24

Half reaction

Oxidation or reduction

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25

Oxidizing agent

Gets reduced

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26

Reducing agent

Gets oxidized

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27

Oxidation numbers rules

Alkali metals: +2, Alkaline metals: +2, Oxygen: usually -2 but -1 in peroxides, Hydrogen: +1 with nonmetals and -1 with metals, Fluoride: always -1

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28

Spontaneous

Strong oxidizing + strong reducing, energetically favourable

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29

Standard cell potential

Let’s us compare reactions

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30

Non-spontaneous

Weak oxidizing + weak reducing, not energetically favourable

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31

Potential difference

Energy delivered by the movement of electrons

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32

Volt

Energy carried by a coulomb of electrons

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33

Ampere

Number of coulombs that travel per second

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34

Coulomb

A bunch of electrons

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35

Electrode

Conductor where half reaction occurs

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36

Anode

ELectrode where oxidation takes place

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37

Cathode

Electrode where reduction takes place

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38

Solutions used

Usually nitrate b/c they dont react

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39

Salt bridge

Allows the movement of ions and balances the charges

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