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AP 1 > Quiz 2 > Flashcards

Quiz 2 Flashcards

1
Q

Define chemistry

A

The science of the structure and interactions of matter

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2
Q

Define matter

A

Anything that occupies space and has a mass

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3
Q

Define mass

A

The amount of matter a substance has

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4
Q

Define weight in relation to mass

A

Weight is the force of gravity acting on a mass

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5
Q

Define chemical elements

A

Building blocks of all matter living and nonliving

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6
Q

Define atoms

A

Smallest unit of matter that retains the properties and characteristics of that element

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7
Q

Atomic number

A

Number of protons in an element

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8
Q

Mass number

A

Sum of protons and neutrons in an element

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9
Q

Define atomic mass/weight

A

Average mass of all naturally occurring isotopes

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10
Q

Define isotopes

A

Atoms of an element that have different numbers of neutrons and therefore a different mass number

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11
Q

Define ion

A

An atom or molecule that gives up or gains an electron and therefore has a charge

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12
Q

Define compounds

A

Contains atoms of 2 or more different elements

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13
Q

Electrolytes

A

Ionic compound that breaks down into cations and anions in a solution

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14
Q

Octet rule

A

An atom needs 8 electrons in its valence shell to be stable. Atoms are more likely to interact if doing so will leaveboth valence shells with 8 elections

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15
Q

What makes noble gases special?

A

They are stable on their own because they have a full valence shell. They don’t need to bond.

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16
Q

Ionic bonds

A

Cations and anions attract each other due to the opposition of charges. Usually exist in solids. Found mostly in teeth, bones

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17
Q

Nonpolar covalent bonds

A

2 or more atoms share electrons evenly. Can form between atoms of the same or different elements. Can share up to 3 pairs of Valence elections

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18
Q

Polar covalent bonds

A

Electrons shared unevenly due to electronegativity. Nucleus of bigger atom attracts the shared electron more strongly so it becomes partially negative. The smaller electron becomes slightly more positive.

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19
Q

Electronegativity

A

The measure of an atom’s ability to attract shared elections to itself.

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20
Q

Hydrogen bonding

A

Weak bond that occurs due to the polarity of polar covalent bonds- not really a solid bond, more of an attraction.results from attraction of oppositely charged sharing of electrons

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21
Q

Free radical

A

Atom or group of atoms with an unpaired election in the outermost shell. Unstable, highly reactive, destructive to nearby molecules. Antioxidants inactivate them.

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22
Q

Radioactivity

A

When unstable atoms spontaneously break themselves down to reach a stable state. Breakdown causes radioactivity.

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23
Q

Half-life

A

Time it takes for half the atoms of a radioactive substance to break down into a more stable form.

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24
Q

Law of conservation of mass

A

Mass cannot be created or destroyed

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25
Q

Law of conservation of energy

A

Energy cannot be created or destroyed) only transferred

26
Q

Potential energy

A

Energy stored by matter due to position (think holding up a ball)• static, waiting to be used.

27
Q

Kinetic energy

A

Associated with matter in motion (think after you let go of the ball and it falls to the ground)

28
Q

Exergonic reactions

A

Reactants start with energy and products have less energy after reaction (catabolic). Extra energy is released.

29
Q

Endergonic reactions

A

Reactants start without energy and products gain energy (anabolic). Energy is required for the reaction. Absorb more energy than is released.

30
Q

Metabolism

A

The sum of all chemical reactions in the body. Coupling of exergonic and endergonic reactions - energy released from exergonic usually used to drive endergonic.

31
Q

Activation energy

A

Energy required for a reaction to occur. Reactions depend on concentration and temperature. High concentration of atoms means there are more atoms available to bond. High temperature makes atoms more around a lot, increasing likelihood of forming bonds.

32
Q

Catalysts

A

Help speed up reactions by lowering amount of activation energy needed to start a reaction. Ex. Enzymes in the body.

33
Q

Synthesis

A

Chemical reaction where the resulting product is bigger than the reactants. Bonds formed. Anabolism. Usually endergonic.

34
Q

Decomposition

A

Chemical reaction where resulting products are smaller than reactants. Bonds broken. Aka catabolism. Usually exergonic.

35
Q

Exchange reactions

A

Ab+cd = ad + BC

36
Q

Reversible reactions

A

Ab ←→ a+b

37
Q

Inorganic vs. Organic compounds

A

Inorganic usually doesn’t contain carbon. Organic always has carbon, usually hydrogen and always covalent bonds. Organic compounds are more complex.

38
Q

H2O has polarity. T/f

A

True

39
Q

Hydrolysis

A

Breakdown of large molecules into simpler ones with H2O

40
Q

Dehydration synthesis

A

2 simple molecules join together, eliminating H2O in the process.

41
Q

Dehydration synthesis vs. Hydrolysis

A

H20 is the product in dehydration synthesis, but the reactant in hydrolysis

42
Q

Ionization

A

The process by which ions are formed by gain or loss of an electron from an atom or molecule.

43
Q

Hydrophilic

A

Dissolves in H20. Has polar covalent bonds.

44
Q

Hydrophobic

A

Not water soluble

45
Q

Mixture

A

Combo of elements or compounds physically blended together but not bound by chemical bonds.

46
Q

Solutions

A

Solutes mixed into a solvent are evenly distributed (transparent)

47
Q

Colloids

A

Size of particles of solvent larger than in a solution so it is opaque. Ex. Milk

48
Q

Suspension

A

Suspended material may mix at the beginning but will settle out. Ex. Muddy water.

49
Q

Concentration

A

How much solute is found in the solvent. Moles per litre (moL/L) = morality

50
Q

Acid

A

Proton donor, pH below 7

51
Q

Base

A

Proton acceptor. pH above 7

52
Q

Salt

A

Electrolytes- acids and bases react to form salts.

53
Q

Buffer systems

A

Used to convert strong acids and bases into weaker ones. they remove or add protons.

54
Q

Carbohydrates

A

Function mainly as a source of chemical energy for generating ATP. Formed via carbon, hydrogen, oxygen.
2:1 H:O. 1 H2O per C. sugars, glycogen, starches, cellulose

55
Q

3 major groups of carbs

A

Monosaccharides, disaccharides, polysaccharides

56
Q

what are simple sugars made up of

A

monosaccharides and disaccharides (combo of 2 monosaccharides through dehydration synthesis). end in -ose.

57
Q

characteristics of simple sugars

A

can be absorbed without need to digest further. use hydrolysis to break down disaccharides and polysaccharides

58
Q

how are saccharides joined together

A

dehydration synthesis

59
Q

polysaccharides

A
  • many monosaccharides joined together through dehydration synthesis
  • glycogen is the main one found in the body. - hydrolysis can break them down into monosaccharides.
  • found in starches
60
Q

where in the body is glycogen stored

A

liver and skeletal muscle

61
Q

what is the storage form of glucose in the body

A

glycogen

62
Q
A

AP 1 (5 decks)

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