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A&P Unit 1 > Chemistry > Flashcards

Chemistry Flashcards

1
Q

Define matter

A

anything that occupies space and has mass

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2
Q

T/F: Weight is a function of mass

A

False; weight is a function of gravity; mass will be the same regardless of gravity

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3
Q

The human body contains how many natural elements?

A

24

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4
Q

Define element

A

a substance that cannot be broken down into smaller substances by ordinary chemical means

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5
Q

What are some examples of solids in the body?

A

bones, teeth

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6
Q

What are some examples of liquids in the body?

A

blood, brain fluid, urine

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7
Q

What are some examples of gases in the body?

A

oxygen, CO2 gas

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8
Q

Define energy

A

the ability to do work; the ability to put matter into motion

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9
Q

Define kinetic energy

A

the energy of work

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10
Q

What is an examples of kinetic energy within the human body?

A

breaking bonds, walking/running

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11
Q

Define potential energy

A

stored energy

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12
Q

What are some examples of potential energy in the body?

A

carbohydrates, bonds between molecules

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13
Q

Define chemical energy

A

energy that is contained in chemical bonds

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14
Q

Bonds _______ energy when they are broken; bonds _______ energy when they are formed

A

release; absorb

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15
Q

Define electrical energy

A

energy that results from the flow of particles

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16
Q

What is an example of electrical energy within the body?

A

cells create electrical currents that allow the heart to contract at just the right time

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17
Q

Define mechanical energy

A

energy required for movement

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18
Q

What is an example of mechanical energy in the body?

A

cellular respiration

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19
Q

Define electromagnetic energy

A

radiant energy

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20
Q

How does electromagnetic energy move?

A

in waves

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21
Q

What is an example of electromagnetic energy in the body?

A

used in MRIs and MRSs

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22
Q

First Law of Thermodynamics states:

A

energy is neither created or destroyed; it can only be transferred from one type to another

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23
Q

Second Law of Thermodynamics states

A

when energy is transferred from one form to another, some is lost as heat

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24
Q

In our bodies, why is beneficial that transfers of energy result in heat?

A

Helps us to maintain our body temperatures

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25
Q

What subatomic particles are found in the nucleus? What are their respective charges?

A

protons (+), neutrons (neutral)

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26
Q

T/F: Electrons take up the most mass in an atom

A

False; the nucleus makes up most of the mass of an atom

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27
Q

What charge does an electron carry?

A

negative

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28
Q

The number of protons in an atom is equal to the number of ________?

A

electrons

29
Q

Atomic mass is equal to the sum of which two subatomic particles?

A

protons and neutrons (because these are what the nucleus is made of which comprises the majority of an atom’s mass - common sense)

30
Q

The atomic number of protons tells you what?

A

the atomic number, the number of electrons

31
Q

What is different about an isotope?

A

it has the same number of protons and electrons as its parent atom, but a different number of neutrons (what is supposed to be neutral is not!)

32
Q

T/F: Isotopes are the most stable form of an element

A

False; they are quite unstable; radioactive

33
Q

What are names used for the outer regions in which electrons move around the nucleus?

A

orbitals, shells, energy levels

34
Q

How many electrons can be held by the first shell? The second shell? The third?

A

2; 8; 8…

35
Q

What is the “octet rule?”

A

after the first shell, orbitals can hold up to 8 electrons

36
Q

What is referred to as the “valence level?”

A

the outermost shell

37
Q

What are valence electrons?

A

electrons orbiting on the outermost shell; can be a full shell or not full shell

38
Q

T/F: A full valence shell means the atom is stable

A

True

39
Q

T/F: A full valence shell means the atom is unstable

A

False; atoms are considered unstable if their outer shells are not full - they want them to be which is why they are unstable!

40
Q

Define chemical reactions

A

combining or breaking apart atoms to form new products with different properties from the originals

41
Q

Essentially, chemical reactions are just the interactions of what?

A

valence electrons

42
Q

How does an electron fill its valence shell?

A

either by giving up/donating electrons, or by accepting/sharing electrons

43
Q

Define molecule and give an example

A

combination of 2 or more atoms from a reaction; can be the same atom twice, or two different atoms (N2, O2, NaCl, etc.)

44
Q

Define compounds and give an example

A

substance that can be broken down into 2 or more atoms by chemical means (NaCl, HCl, C6H12C6, etc.)

45
Q

T/F: All compounds are molecules but not all molecules are compounds

A

True; molecules can be a combination of two of the same atoms (N2), whereas compounds must be composed of at least two different atoms

46
Q

What is an ionic bond?

A

occurs when ions of different charges are attracted to each other; one atom donates electrons while the other accepts them

47
Q

Define cation

A

positively-charged ions which act as electron donors; have more protons than electrons, thus the positive charge

48
Q

Define anion

A

negatively-charged ions which act as electron acceptors; have more electrons than protons, thus the negative charge

49
Q

Ions in our bodies are called what?

A

salts and electrolytes

50
Q

What happens in a covalent bond?

A

electrons are shared between atoms

51
Q

What types of bonds can be formed in a covalent bond?

A

single, double, and triple bonds; single are the weakest, triple are the hardest to break

52
Q

What is a hydrogen bond?

A

a weak attractive force between a hydrogen atom in one molecule and an electronegative atom in a different molecule; super weak force

53
Q

T/F: Hydrogen bonds are the strongest bonds

A

False; first, hydrogen bonds are not technically bonds, they are attractive forces; second, they are incredibly weak

54
Q

List the 7 possible types of reactions

A

synthesis, decomposition, exchange, oxidation-reduction, reversible, exergonic, and endergonic

55
Q

What is a synthesis reaction? Give an example

A

when smaller things combine to make bigger things; ex: 2Na + Cl2 –> 2NaCl

56
Q

What is a decomposition reaction? Give an example.

A

breaking big things down into small things; ex: digestion, 2NaOH –> Na2O + H2O

57
Q

What is an exchange reaction? Give an example.

A

a cation from one reactant reacts with the anion of the other reactant; ex: NaCl + AgNO3 –> NaNO3 + AgCl

58
Q

What is an oxidation-reduction reaction? Give an example.

A

a subtype of an exchange reaction in which a swapping of ions occurs (oxidized atom donates electrons and becomes (+) while a reduced atom accepts electrons and becomes (-)); ex: Fe + O2 –H2O–> Fe2O3

59
Q

What is a reversible reaction? Give an example.

A

the products can revert back to the reactants, however there is typically a direction that is preferred; ex: H2 + I2 <—-> 2HI

60
Q

What is an exergonic reaction? Give an example.

A

products are at a lower energy level than the reactants (energy was released); ex: bond breaking

61
Q

What is an endergonic reaction? Give an example.

A

products are at a higher energy level than reactants (energy was absorbed); ex: bond formation

62
Q

Which reaction types are anabolic?

A

synthesis, endergonic

63
Q

Which reaction types are catabolic?

A

decomposition, exergonic

64
Q

Which reaction types are both anabolic and catabolic?

A

exchange, oxidation-reduction

65
Q

Which reaction types are neither anabolic nor catabolic?

A

reversible

66
Q

What is Collision Theory?

A

an explanation for why and how chemical reactions occur; essentially, if all particles are in constant motion, then they are continually colliding with one another. If collisions create activation energy, then bonds can be broken and formed as a result of these collisions

67
Q

What is activation energy?

A

the amount of collision energy needed for a chemical reaction to take place; the amount of energy it takes to rearrange the electrons in a molecule

68
Q

What are the 6 factors that can affect the rate of chemical reactions?

A

velocity, temperature, energy, size, concentration, and catalysts

A&P Unit 1 (5 decks)

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