Unit 1

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59 Terms

1
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List and describe the three states of matter

  • Solid: definite Shape and volume; molecules tightly packed and vibrate

  • Liquid: definite volume but no definite shape; molecules loosely packed and flow past each other

  • Gas: No definite volume or shape; molecules very far apart and move freely

2
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Define kinetic particle theory.

Describes all matter as a collection of particles that are in constant random motion.

3
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What happens to water molecules in their solid, liquid, and gas state.

  • To form ice, water molecules are arranged in a lattice

  • Liquid water molecules take the shape of container but cannot be compressed

• Water molecules in a gaseous state is water vapor

4
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List and describe the process in which matter moves through the three states.

Melting - change from solid to liquid

Freezing - liquid to solid

Evaporation - liquid to gas

Condensation - gas to liquid

Deposition- gas to solid

Sublimation- solid to gas

5
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Explain the subatomic structure of atoms.

Atoms are made up of protons that are located in the nucleus, neutrons which are also in the nucleus and electrons in the orbital

6
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What is the charge of a proton, neutron and electron?

Protons have a positive charge, neutrons have no charge and electrons have a negative charge.

7
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What is the mass of a proton, neutron and electron?

Protons and neutrons have a mass of 1 amu, electrons have a mass on zero amu.

8
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How many electrons can each valence shell hold?

The first shell can hold 2 electrons and the rest hold 8

9
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When are atoms most stable?

Atoms are most stable when all of the shells are full.

10
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What is the differenc between and element, compound and a mixture?

Elements are made of one type of atom only. A compound is made of two or more types of atoms that are chemically bonded. The only differences with mixtures is that they’re not chemically combined.

11
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What does it mean for compounds to have emergent properties?

Properties of compounds can be very different than those of the individual elements.

12
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What are the bonds and how are they broken?

Bonds are lasting attractions between two or more atoms, ions, or molecules. They can only be broken by chemical reactions.

13
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What is a covalent bond?

Covalent bonds are between tow nonmetal atoms and electrons are shared.

14
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What is an ionic bond?

Ionic bonds form between a metal and nonmetal atom by transferring electrons. (forms ions)

15
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What is a hydrogen bond?

Weaker type of covalent bond between molecules containing a hydrogen atom bonded to oxygen, nitrogen or fluorine.

16
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What is an example of a covalent bond and sketch a model of the interaction between electrons?

Cl2 is an example of a covalent bond.

17
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What is an example of an ionic bond and sketch a model of the interaction between electrons?

Lithium and chlorine is an example of an ionic bond.

18
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Water is an example of a hydrogen bond, sketch a water molecule below.

H2O is an example of a hydrogen bond.

19
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What are the chemical names and formulas of salt compounds found in seawater?

Sodium Chloride (NaCl)

Magnesium Sulfate (MgS04)

Calcium Carbonate (CaC03)

20
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What are the important covalent molecules found in seawater (be able to know them by name and what they look like

Water

Carbon Dioxide

Oxygen

Sulfur Dioxide

Glucose

21
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What are the important ionic substances found in seawater (be able to know them by name and what they look like)

Sodium Chloride

Magnesium Sulfate

Calcium Carbonate

22
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What makes water polar?

Electrons are shared unequally between oxygen and hydrogen molecules because of oxygens stronger attraction, leading to hydrogen having a positive charge and oxygen having a negative charge.

23
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Define cohesion

Cohesion - the attraction between the same types of molecules

24
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Define adhesion

Adhesion - the attraction between different types of molecules

25
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What is the difference between the density of liquid water molecules and solid water molecules? Why is this difference in density important?

The crystalline lattice formed in solid water molecules creates more space between molecules, therefore solid water is less dense than liquid water. Since ice is less dense it floats on the surface of the water and traps heat in the water.

26
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What is the difference between a solvent and solute?

Solutes are the substances being dissolved.

Solvents are the substances that dissolve something else.

27
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Define dissolution

Dissolution - the process of being dissolved.

28
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Define solubility

Solubility - the ability of a solute to dissolve within a solvent.

29
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Why is water considered the universal solvent?

Water molecules surround each ion to dissolve it and is able to dissolve many polar and ionic substances.

30
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How is NaCL (salt) dissolved in water?

The electrostatic charge of NaCl attracts water which breaks the ionic bond.

31
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What is the relationship between temperature and the rate of dissolution of salt in water?

As temperature rises, the rate of dissolution is salt water increases.

32
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Describe the waters latent heat of vaporization?

Water has a high latent heat of vaporization (liquid to gas) because a lot of heat energy is required to break hydrogen bonds.

33
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Describe waters high specific heat capacity and what causes it?

Waters high specific heat capacity is caused by the strength and amount of hydrogen bonds present in the water.

34
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Why is it important that water has a high specific heat capacity?

It regulates temperatures so that they don’t get too high (acts as a buffer). It helps maintain stable body temperatures and moderates climate.

35
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Describe the following stages of the water cycle: evaporation, condensation, precipitation, transpiration, percolation/infiltration, and ocean accumulation.

Evaporation is when liquid is changes into a gas, condensation forms clouds when water vapor cools into a liquid, transpiration is evaporation from the leaves of plants, precipitation is water falling from the sky, percolation - water moves through soil layers and ocean accumulation is when water pools in large bodies.

36
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Define salinity and what units are used to measure it.

Salinity - measure of the concentration of dissolved salts in seawater (measured in parts per thousand, ppt)

37
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What is the average salinity of the ocean and how can it vary based on precipitation and evaporation?

Average salinity of ocean is 35 ppt. Precipitation can lower salinity by diluting salt. Evaporation can raise salinity by removing water and leaving salt behind.

38
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Define hypersaline.

Hypersaline - salt concentration greater than 35 ppt

39
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What happens to the freezing point of water when salinity increases

Increased salinity results in lower freezing point.

40
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Define halocline.

Halocline - a layer of water below the mixed surface layer where a rapid change in salinity can be measured as depth increases.

41
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What is the general relationship between salinity and depth? How does this relationship affect the density of water? What is and exception to this relationship?

Generally, salinity increases with depth. Density increases with salinity. Exception: tropical seas where temps are high result in increased evaporation and a salty top layer.

42
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What is the relationship between water temperature and depth? How does this relationship affect the density of water?

Water temperature decreases with depth because the amount of sunlight decreases with depth and as temperature decreases, density increases because cold water is denser and sinks.

43
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Define thermocline.

thermocline - a layer between two layers of water where temperature abruptly changes with depth.

44
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What is the difference between water temperatures in tropical vs. polar regions?

Tropical seas have a steeper temperature gradient from the surface to sea floor. Polar seas have surface temps close to freezing and remain consistent with increasing depth.

45
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What is the relationship between water pressure and depth? How does this relationship affect the density of water?

Water pressure increases with depth and pressure increases density because molecules are pushed closer together (more mass, same volume)

46
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Define pycnocline.

Pycnocline - an area of water where density changes quickly with depth.

47
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What can affect the presence or absence of thermoclines, haloclines, and pycnoclines?

These three are more prevalent in calm waters. Mixing caused by waves and winds (rough stormy waters) cause them to disappear.

48
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What is the relationship between light penetration in water and depth?

Light penetration decreases with depth.

49
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What is the formula to calculate density?

Density = mass (kg) / volume (m cubed)

50
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What is an acid? What is the number range for acids on the pH scale?

Acid - substance that breaks apart in water to form a hydrogen ion(H+). More hydrogen ions = stronger acid. Range = 0-6

51
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What is a base? What is the number range for bases on the pH scale

Base - substance that breaks apart in water to form a hydroxide ion (OH-)

52
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What is a neutral? What is the number range for neutrals on the pH scale?

Neutral - pH of 7; not acidic or basic; equal # of Hydrogen ion and Hydroxide ion.

53
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List and describe three ways that pH can be measured.

pH probe - gives a clear number

Litmus paper - turns color based on pH

Universal indicator - turns the solution a certain color

54
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What is the relationship between gases in the ocean and the atmosphere?

The gases are at equilibrium. This balance is caused by turbulence and wave action.

55
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What is the difference between the solubility of carbon dioxide and oxygen in water?

Carbon Dioxide is very soluble in water because it forms carbonic acid. Oxygen is not as soluble because it doesn’t chemically combine with water molecules.

56
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How does temperature affect the solubility of gases in water?

Cold temps dissolve more gas than warm temps because warm temps evaporate dissolved gas molecules from the surface.

57
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How does atmospheric pressure affect the solubility of gases in water?

Gas solubility increases when atmospheric pressure increases. Atmospheric pressure pushes more gas molecules to dissolve.

58
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How does water pressure affect the solubility of gases in water?

As depth increases so does pressure. Increased water pressure increases gas solubility as well because pressure causes molecules to be closer together.

59
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How does salinity affect the solubility of gases in water?

As salinity decreases, gas solubility increases because less salt is in the way to interfere with water molecules dissolving the gas.