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Chemistry 1100 > Chapter 5 - Water > Flashcards

Chapter 5 - Water Flashcards

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1
Q

What happens to water when it freezes?

A

it expands

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2
Q

What is specific heat? Is it high or low for water?

A

how much energy it takes to raise 1 gram of a substance 1 degree celsius
high for water (1 cal/(g x degrees celsius)

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3
Q

What is heat of fusion? Is it high or low for water?

A

the amount of energy it takes to change a substance from solid to liquid
high for water

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4
Q

What is heat of vaporization? Is it high or low for water?

A

the amount of energy it takes to change a substance from liquid to gas
high for water

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5
Q

What are the properties of water?

A

standard for celsius
18.02 g/mol
boiling point 100 degrees celsius

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6
Q

What is the structure of water?

A

H-O-H

  • bent
  • two O-H bonds (covalent, shared electrons)
  • -> electrons not shared equally, more time spent around oxygen atoms
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7
Q

What is electronegativity (EN)?

A

how attractive an atom is to electrons (ex. O is more electronegative than H)

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8
Q

Properties of electronegativity

A
  • atoms further right on PT have stronger electron pull
  • going down the PT has less electron pull
    (exception: noble gases don’t want more electrons or to have to give them up - all substances want to be like noble gases)
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9
Q

Electronegativity Scale

A 
H: 2.1
F: 4
Cl: 3
go left and drop .5 each atom from F
go right from Na and add .3, right from P add .4
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10
Q

Water’s O-H bonds

A

O: 3.5, H: 2.1
more electrons around O –> O has partial negative charge, H has partial positive charge (polar covalent bond: opposite partial charge at either end of molecule)

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11
Q

What are hydrogen bonds?

A

attraction between two different molecules

  • weak bonds: covalent are 10 times stronger
  • result of bonds: H2O sticks together
  • -> liquid, high boiling/melting temp, etc because H-bonds take energy to break
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12
Q

What molecules create hydrogen bonds?

A

N-H
O-H
H-F (only hydrofluoric acid)

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13
Q

Why does water expand when freezing?

A
  • hydrogen bonds: freeze–>crystal structure
  • atoms can’t get close due to bonds
  • -> result: ice, less dense than water
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14
Q

What is density?

A

measurement of how much matter is in a certain volume

  • mass per unit volume (kg/m^3, g/L, g/cm^3)
  • -> water: 1 g/cm^3, ice: .92 g/cm^3 (however, solid is usually denser)
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15
Q

Division of Earth’s water

A

fresh water = 2.6% (.01% ground/surface water, 2.59% glaciers/ice caps)
salt water = 97.4%

surface water: oceans, lakes, rivers, glaciers (often contaminated)
ground water: wells, rural (contaminant-free, ground filters water)

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16
Q

Water Consumption

A

drinking: 1.5 gal/day
washing/flushing: 40 gal/day
typical westerner: 100x body mass/day

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17
Q

Water Use

A

80% power plants, irrigation/agriculture

20% other uses (cooking, cleaning, sewage, drinking)

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18
Q

What is an aquifer?

A

water trapped in sand/gravel

  • if this gets contaminated = very bad
  • depleting quickly because farmers are taking too much
  • -> we use 48 in/yr, replenished by rainfall by 2 in/yr
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19
Q

What is a solvent?

A

dissolves other compounds

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20
Q

What is a solute?

A

stuff being dissolved

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21
Q

What is a solution?

A

solvent + solute

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22
Q

What is an aqueous solution?

A

water is the solvent

ex. saline solution: solvent is water, solute is salt

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23
Q

What are ions?

A

charged particles

24
Q

What is concentration?

A

the amount of solute per volume of solvent

“[…..]”: “concentration of”

25
Q

How do you measure concentration?

A
  1. percent by mass
  2. parts per million (grams/million grams, mg/L)
  3. parts per billion (grams/billion grams, micrograms/L)
26
Q

What is molarity? How do you find it?

A

moles per liter

  1. convert g to mol
  2. convert volume to L
  3. divide mol by L
27
Q

What are electrolytes?

A

substances that conduct electricity when dissolved in water
Ex.
-pure distilled water (non-conducting)
-sugar dissolved in water (non-conducting –> non-electrolyte)
-NaCl dissolved in water (conducting –> electrolyte)

28
Q

Conductivity is due to ____ in a solution

A

ions

  • more ions = better conduction
  • electrolyte = ionized
29
Q

What is an ionic compound made of?

A

cations and anions

30
Q

What are polyatomic ions?

A

where an ion has a different number of protons or electrons because they are filling and octet
*know name, formula, and charge for test (CHEAT SHEET)

31
Q

What are ionic bonds?

A

bonds that hold ionic compounds together

-opposite charges attract (cations and anions)

32
Q

How can you tell is something is an ionic compound?

A

cation: metal or ammonium (NH4+)
anion: nonmetals and polyatomic anions
1. metal + nonmetal
2. metal + polyatomic ion
3. ammonium + nonmetal
4. ammonium + polyatomic ion

33
Q

How to name ionic compounds

A
  1. name cation as element
  2. name anion, add “ide” to element name
  3. name the polyatomic ion of it applies (don’t mess with ending)
34
Q

Periodic Table charges

A

metals: 1A: +1, 2A: +2, 3A: +3, 4A: +4
nonmetals: 4A: -4, 5A: -3, 6A: -2, 7A: -1
Know these: Ag: +1, Cd: +2, Zn: +2

35
Q

What is formula for Sodium Chloride?

A

NaCl

36
Q

What is formula for Magnesium Bromide?

A

MgBr2

37
Q

What is the formula for Calcium Oxide?

A

CaO

38
Q

What is the name for BaCl2?

A

Barium chloride

39
Q

What is the name for K2O?

A

potassium oxide

40
Q

What is the name for Mg(OH)2?

A

magnesium hydroxide

41
Q

What is the name for KNO3?

A

potassium nitrate

42
Q

How do you label for charges?

A

roman numerals

43
Q

what is the name of FeCl2?

A

2 Cl = -2, so Fe = +2

iron (II) chloride

44
Q

what is the name of FeCl3?

A

3 Cl = -3, so Fe = +3

iron (III) chloride

45
Q

what is the name of Cr2S3?

A 
3 S (-2) = -6, so 2 Cr = +6
chromium (III) sulfide
46
Q

what is the symbolic name of Manganese (IV) oxide?

A

Mn = +4, O = -2

Mn2O4

47
Q

Dissolving sodium chloride in water

A
  • partial charges in H20 will still be attracted to full formal charges of other molecules
  • created energy through hydrogen bonds makes up for the bonds are broken in NaCl
48
Q

What are insoluble ionics?

A

ion attraction that is too great for H2O to break therefore won’t dissolve (much)

49
Q

What are solvable covalents?

A

ex. sugar, ethanol (covalent compounds, soluble, non-electrolytes)
- have O-H groups (hydroxyl), hydrogen bond with water

50
Q

Consumption of pollutants

A

polar: go into bloodstream (polar environment) are are filtered through kidneys
non-polar: go to fat cells (non-polar environment) and will build up because they are not filtered out
–> less of these

51
Q

What are some mineral concerns of water?

A

Ca: nutrient that makes water hard
Nitrates: agricultural runoff, cause “blue baby” syndrome (soluble, hard to get out of water)
Lead, Chlorine: toxic
Na: cause high blood pressure

52
Q

How to make potable water?

A
  1. Screen: large objects
  2. Al(OH)3: sticks to dirt/clay (insoluble)
  3. Chlorination: kill bacteria/virus, bad taste/smell, toxic by-products (Cl is toxic but not on a drastic level)
53
Q

What is distillation?

A

liquid solution is heated, vapors are condensed and collected (expensive because you have to use solar panels to heat water)

54
Q

What is desalinization?

A

a process that removes ions from salt water

55
Q

What is osmosis?

A

water goes through a semipermeable membrane (wall with holes that only H2O molecules can pass through) from a solution that is LESS concentrated to a solution that is MORE concentrated

56
Q

What is reverse osmosis?

A

forcing water through a semipermeable membrane from a solution that is MORE concentrated to a solution that is LESS concentrated (expensive because you must use high pressure pump to do this)

Chemistry 1100 (11 decks)

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