Chemistry

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53 Terms

1

Open System

Allows energy and matter to cross the systems boundary (tree)

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2

Closed System

Allows only energy but no matter to cross the boundary (earth)

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3

Isolated Systems

Allows neither energy nor matter to flow across the boundary

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4

Atmosphere's layers

troposphere, stratosphere, mesosphere, thermosphere

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5

Troposphere

Lowest layer of the atmosphere where we find weather

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6

Stratosphere

10-50 km above sea level, has the Ozon layer (protects organisms)

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7

Mesosphere

50-80km

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8

Thermosphere

80+km

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9

Lithosphere

Is the solid portions of earth (above semi fluid upper mantle)

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10

Hydrosphere

All water of earth (on the surface area and underground)

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11

Biosphere

Absorbs energy

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12

Reflection

Change the sun ray's direction

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13

Absorption

Energy is converted into another form of energy

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14

Albedo

Ability of a surface to reflect light (higher the Albedo the more it reflects)

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15

Net radiation budget

Difference between the amount of incoming and outgoing radiation (net budget = incoming - outgoing)

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16

How much solar energy is absorbed by land and ocean

49%

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17

How much solar is absorbed reflected and scattered

42%

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18

reflected by earths surface

9%

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19

gases that absorb infrared radiation

water, co2, ch4 (methane), n20 (nitrous oxide), ozon, halocarbon

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20

Photosynthesis

carbon is absorbed through plants

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21

cellular respiration

carbon released into the atmosphere by terrestrial and aquatic living

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22

Photosynthesis (compound)

carbon dioxide + water = glucose + oxygen

CO2 + H2O = C6H12O6 + O2

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23

Cellular respiration (compound)

Glucose + oxygen = carbon dioxide + water

C6H12O6 + O2 = CO2 + H2O

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24

combustion (compound)

Methane + oxygen = carbon dioxide + water

CH4 + O2 = CO2 + H2O

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25

Dalton

Believed all atoms are smart particles of matter. Billiard ball model

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26

Bohr

electrons surrounded the nucleus in specific (quantized) energy levels

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27

JJ Thomson

Atoms are positive spheres embedded with negative charged atoms (plum pudding model)

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28

Ruther Ford

Gold foil experiment. Believed most atoms are empty space with tiny positively charged nucleus and negatively charged electrons orbit the positively charged nucleus (planetary model)

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29

Democritus

Proposed the idea that matter was made up of tiny particles that could not be further subdivided

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30

Aristotle

Proposed (all matter) was made up of four elements. He also proposed matter was infinitely divisible

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31

Mixture

Matter that can be separated by physical means, does not have a definite composition

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32

Heterogeneous

(Mechanical mixtures) Different components of mixtures are visible. Component is variable (salad dressing)

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33

Homogeneous

(solution) -different components are not visible (ice tea)

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34

pure mixture

matter that has a definite composition (chem formula)

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35

Element

Cannot chemically be broken down (is on period table) nor further broken down

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36

Compound

Two or more elements that are chemically combined (can be

separated into simpler substances)

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37

Monatomic

Element type: Single atoms (Li, Na, Mg)

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38

Molecular

Combination of two or more atoms (P4, S8, I2, Br2)

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39

Compound

Two or more elements chemically combined. Different properties than elements

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40

Law of definite proportions

Always has same ratios of atoms (water is always H2O and never anything else)

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41

Parts of Atom

Proton, Neutron, Electron

<p>Proton, Neutron, Electron</p>
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42

Metalloids

Have properties between metal and non metals

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43

Isotopes

Atoms of the same element that have the same number of protons but different number of neutrons ( C-12, C-13, C-14)

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44

Ions

stable, unequal # of P+ and E- there are

two types Cation and anions

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45

Atoms

Unstable (want to be stable),

equal #p+ and e-

form ion naturally by losing or gaining e-

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46

outlet rule

They form ions in order to have a stable outtering

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47

Ionic

Complete transfer of 1 or more electron from one atom to another

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48

Covalent

some valence electrons are shared between atoms

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49

Metallic

Holds atoms of metal together

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50

ionic bonds

usually solid at room temp

formed by a transfer of e- from one atom to another

between metals and none metals

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51

Charged atom

when a atom gains or loses a e- they become charged

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52

metal atoms/ions

loses e- and become positively charged

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53

non metal atoms/ions

gain e- and become neg charged called ANION

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