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Biology > Ch.2 Chemistry > Flashcards

Ch.2 Chemistry Flashcards

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1
Q

Matter

A

Anything that takes up space and has mass

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2
Q

What is an Element?

A

A substance that can not be broken into other substances by chemical reactions

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3
Q

Emergent property

A

I would say, that emergent properties are properties that emerge as a function of interactions of real things.

As things come together more properties are present

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4
Q

6 most common elements in life

A

CHONPS

Carbon, hydrogen, oxygen, nitrogen, phosphorous, sulphur

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5
Q

Trace elements

A

Required by organisms but only in small amounts

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6
Q

What makes elements different from each other?

A

The number of protons

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7
Q

Atom

  • subatomic particles
  • what makes up the nucleus?
  • mostly…
A

The smallest unit of matter that still retains the properties of an element

  • protons, neutrons, electrons
  • tightly packed protons and neutrons
  • empty space
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8
Q

Electrons

A

Float around the nucleus in the “electron cloud” attracted to the protons in the nucleus making the atom neutral and keeping the atoms near the nucleus

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9
Q

Electron shells

  • Max electrons per shell
  • how to know # of valence electrons
A

1st- 2
2nd- 8
3rd- 18
- must fill up max # before moving on to next shell, amount on outer shell = valance electrons

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10
Q

How to find number of…

  • electrons
  • protons
  • neutrons
A
  • atomic number
  • atomic number
  • atomic mass - atomic number
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11
Q

Atomic mass

A 
Number of protons + number of neutrons 
Weighted average (each proton and neutron =1 unit (dalton) and electron are too small to affect weight, so adding amount is the same as calculating weight)
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12
Q

Why do atoms bond

A

They want to complete valence shell

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13
Q

Atomic number

A

Number of protons (each atom is different)

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14
Q

Ion
Cation
Anion

A 
A charged atom (added or lost electron (ionic bond)
Positive ion (lost electron)
Negative ion (added electron)
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15
Q

Hydrogen vs. other atoms in regards to valence shell

A

Hydrogen only needs 1 atom to fill up its shell (it’s on the first shell) every other atom needs 8

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16
Q

Ionic bond

Why do the atoms stay near each other

A

One atom steals an electron from the other.
The “stealer” becomes negative so other atom is positive and they are attracted to each other due to the opposite charges.

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17
Q

Isotopes

A

Atoms of the same element with different numbers of neutrons

- identified by mass, ex. Carbon-14

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18
Q

Calcium atomic number = 20

Ca+2
How many protons?
How many electrons?

A

20

18

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19
Q

Energy
Potential energy
-electrons potential energy comes from…

A
  • the ability to do work
  • the energy that matter stores because of its position or location
  • electrons attracted to the nucleus so the further away they are the more potential energy they have
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20
Q

How to find number of valence electrons by looking at periodic table?

A

Column number

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21
Q

Inert gases

A

Have a full valence shell so don’t interact with other elements

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22
Q

How are atoms in a compound held together?

A

Chemical bonds between the

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23
Q

Orbital?

A

The complex 3D path an electron has orbiting the nucleus

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24
Q

Chemical compounds

A

A substance formed by the chemical combination of 2 or more electrons in definite proportions

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25
Q

What makes carbon special?

A

Only makes covalent bonds

Needs 4 bonds b/c it already has 4 electrons

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26
Q

What makes hydrogen special?

A

Only forms 1 bond

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27
Q

Covalent bond

-molecule?

A

When 2 atoms share a pair of electrons so atom travels through both nucleuses
-2 or more atoms held together through covalent bonds

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28
Q

Single bond
Double bond
Triple bond

A

2 electrons shared
3 shared electrons
6 shared electrons

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29
Q

Van der Waals force

A

Slight attraction that develops between oppositely charged regions of near by molecules.

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30
Q

Polar covalent bonds

Non polar covalent bonds

A

When one atom has a greater attraction to the electron giving both atoms a charge

Both atoms pull equally on the electron, no charge

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31
Q

Hydrogen bonds

A

Occur between polar covalent molecules

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32
Q

Electron negativity

A

The attraction of an atom for the electrons in a covalent bond

33
Q

Ionic bond

What causes the atoms to stay together then?

A

One electron pull is so much greater that the other, the electron is completely transferred
- now both atoms are charged so the attraction between oppositely charged forces (Van der Waals) keeps them together

34
Q

Ion

A

An atom loses or gains an electron it becomes charged, a charged atom is an ion

35
Q

Ionic compound

A

A compound formed through ionic bonds

36
Q

Hydrogen bond

A

When a hydrogen atom that is all ready bonded with a highly electronegative atom is strongly attracted to another strongly electronegative atom
- the first bond makes the hydrogen atom polar so it’s attracted to another polar atom

37
Q

Chemical reaction

  • reactants
  • products
A

Chemical bonds are broken and new ones are formed. Making a new arrangement of atoms.

  • starting molecules
  • end molecules
38
Q

Hydrophobic

A

Does not adhere to water

39
Q

O-H is a ________ bond

A

Polar covalent

40
Q

Specialness of water molecules

A

Due to hydrogen bonding…

A water molecule is polar with opposite ends having opposite charges. So water attracts to anything polar

41
Q

Cohesion

A

An attraction between molecules so the same substance

-surface tension

42
Q

Adhesion

A

Attraction between molecules of different substances

43
Q

Why does water go up plants?

A

Adhesion and cohesion.
The water adheres to the wall of the plant and coheres together. The water is all attached throughout the plant so when water is evaporated off the edge of a leaf it pulls all the molecules (cohesion) up with it

44
Q

How does water moderate temperatures on earth?

A

Water stabilizes air temps by absorbing heat and releasing it based on the temp. With only slight changes to the waters temp

45
Q

Evaporative cooling

A

As a liquid evaporates, the surface left behind is cool. So the hot molecules .eave the water and the cool ones remain. (Why sweating keeps u cool)

46
Q

Why don’t lakes freeze over?

A

Ice floats. If water froze from bottom up lakes and oceans would be frozen solid becaus wide would freeze then keep freezing on top of itself. But when ice floats it basically protects the water under it from floating

47
Q

Solute:
Solvent:
Saturated:
Suspension:

A
  • substance being dissolved
  • substance solute is dissolved in
  • when the solvent has dissolved all solute possible
  • materials that do not dissolve in water
48
Q

Aqueous solution

A

Solution with water as solvent

49
Q

Hydrophilic

Hydrophobic

A

A substance with an a affinity for water (dominated by ionic bonds)
-substances with no affinity for water (equal sharing of electrons when bonding)

50
Q

Acid vs. base

-buffers

A

Acid is a H+ and base is OH-

  • weak acids or bases that react with strong strings acids and bases to prevent sudden changes in pH
  • acids 0-6, bases 8-14
51
Q

Acid percipitation

A

When rain, snow, or fog has a pH more acidic then 5.6, due to extreme assault on water quality

52
Q

Organic chemistry

A

The study of carbon compounds

53
Q

REMEBER the TOTAL number of electrons is different the the number of VALENCE electrons
How?

A

Total is amount counting every shell and valence is just the outer shell
(2 on first ring then add 8 each ring (2,10,18)

54
Q

Carbon always forms _____ bonds

A

Covalent

55
Q

Isomers

A

Compounds that have the same molecular formula but different structures therefore different chemical properties

56
Q

Functional groups

A

Attachments that replace one or more hydrogen atoms to the carbon skeleton if the atom

57
Q

Hydroxyl group

A

A hydrogen atom forms a polar covalent bond with an oxygen atom

58
Q

Saccharide=
Monosaccharide=
Disaccharide=

A
  • sugar
  • 1 sugar molecule
  • 2 sugar molecules
59
Q

Why does sugar absorb water?

A

It forms polar bonds which attach to the water molecules (also polar)

60
Q

Macromolecules

-4 major types

A

Molecules made from thousands or even hundreds of thousands atoms. Monomers join together

  • carbohydrates
  • protein
  • nucleus acid
  • lipids
61
Q

How are the monomers in macromolecules held together

A

Condensation reaction

Dehydration synthesis

62
Q

How are carbohydrates produced

A

Photosynthesis

63
Q

What atoms are carbohydrates made out of

A

Made of a carbon 2 hydrogen and a oxygen atom

64
Q

Function if carbohydrate

A

Energy/ fuel

Extra sugar storage

65
Q

Hydrolysis

A

How to breakdown polymers, sugars separate by adding water (H2O)

66
Q

Polysaccharides function

A

Energy storage

Building material

67
Q

Starch

A

Storage polysaccharide composed entirely of glucose monomers

68
Q

Lipids, hydrophobic or hydroliphic?

A

Hydrophobic

69
Q

Function of lipids

A

Store energy or waterproof coverings of membrane

70
Q

Saturated

A

Contains max number of hydrogen atoms, all single bonds

71
Q

Unsaturated

Polyunsaturated

A
  • 1 carbon double bond

- more then 1 carbon double bond

72
Q

Fatty acid

A

Carboxyl group attached o a long carbon skeleton

73
Q

Trigylcerol

A

3 fatty acids (solid as a fat liquid as an oil)

74
Q

Fat function

A

Energy storage
Cushions vital organs
Insulation

75
Q

Phospholipids

  • where are they?
  • What are they made of?
A
  • cell membrane (double layer)
  • 2 fatty acid tails attached to a glycerol and a phosphate group (phosphate group has a negative charge, fatty acids have no charge)
76
Q

Steroid

-function

A

Molecule made of 4 rings of carbon, precursor to a hormone

-prevents van der Waals forces

77
Q

Protein

A

A macromolecule with amino acids as the monomer
-All protein molecules are made up of the same 20 amino acids (aka peptide, making a protein a polypeptide) in different orders and lengths

78
Q

What differentiates the amino acids

-How are they held together in a protein

A

The R groups, some are polar, some no polar, some hydroliphic….
-Dehydration synthesis

79
Q

Are enzymes reusable?

A

Yes

Biology (10 decks)

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