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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
What subatomic particles are found in the nucleus? What are their respective charges?
protons (+), neutrons (neutral)
26
T/F: Electrons take up the most mass in an atom
False; the nucleus makes up most of the mass of an atom
27
What charge does an electron carry?
negative
28
The number of protons in an atom is equal to the number of ________?
electrons
29
Atomic mass is equal to the sum of which two subatomic particles?
protons and neutrons (because these are what the nucleus is made of which comprises the majority of an atom's mass - common sense)
30
The atomic number of protons tells you what?
the atomic number, the number of electrons
31
What is different about an isotope?
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
T/F: Isotopes are the most stable form of an element
False; they are quite unstable; radioactive
33
What are names used for the outer regions in which electrons move around the nucleus?
orbitals, shells, energy levels
34
How many electrons can be held by the first shell? The second shell? The third?
2; 8; 8...
35
What is the "octet rule?"
after the first shell, orbitals can hold up to 8 electrons
36
What is referred to as the "valence level?"
the outermost shell
37
What are valence electrons?
electrons orbiting on the outermost shell; can be a full shell or not full shell
38
T/F: A full valence shell means the atom is stable
True
39
T/F: A full valence shell means the atom is unstable
False; atoms are considered unstable if their outer shells are not full - they want them to be which is why they are unstable!
40
Define chemical reactions
combining or breaking apart atoms to form new products with different properties from the originals
41
Essentially, chemical reactions are just the interactions of what?
valence electrons
42
How does an electron fill its valence shell?
either by giving up/donating electrons, or by accepting/sharing electrons
43
Define molecule and give an example
combination of 2 or more atoms from a reaction; can be the same atom twice, or two different atoms (N2, O2, NaCl, etc.)
44
Define compounds and give an example
substance that can be broken down into 2 or more atoms by chemical means (NaCl, HCl, C6H12C6, etc.)
45
T/F: All compounds are molecules but not all molecules are compounds
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
What is an ionic bond?
occurs when ions of different charges are attracted to each other; one atom donates electrons while the other accepts them
47
Define cation
positively-charged ions which act as electron donors; have more protons than electrons, thus the positive charge
48
Define anion
negatively-charged ions which act as electron acceptors; have more electrons than protons, thus the negative charge
49
Ions in our bodies are called what?
salts and electrolytes
50
What happens in a covalent bond?
electrons are shared between atoms
51
What types of bonds can be formed in a covalent bond?
single, double, and triple bonds; single are the weakest, triple are the hardest to break
52
What is a hydrogen bond?
a weak attractive force between a hydrogen atom in one molecule and an electronegative atom in a different molecule; super weak force
53
T/F: Hydrogen bonds are the strongest bonds
False; first, hydrogen bonds are not technically bonds, they are attractive forces; second, they are incredibly weak
54
List the 7 possible types of reactions
synthesis, decomposition, exchange, oxidation-reduction, reversible, exergonic, and endergonic
55
What is a synthesis reaction? Give an example
when smaller things combine to make bigger things; ex: 2Na + Cl2 --> 2NaCl
56
What is a decomposition reaction? Give an example.
breaking big things down into small things; ex: digestion, 2NaOH --> Na2O + H2O
57
What is an exchange reaction? Give an example.
a cation from one reactant reacts with the anion of the other reactant; ex: NaCl + AgNO3 --> NaNO3 + AgCl
58
What is an oxidation-reduction reaction? Give an example.
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
What is a reversible reaction? Give an example.
the products can revert back to the reactants, however there is typically a direction that is preferred; ex: H2 + I2 <----> 2HI
60
What is an exergonic reaction? Give an example.
products are at a lower energy level than the reactants (energy was released); ex: bond breaking
61
What is an endergonic reaction? Give an example.
products are at a higher energy level than reactants (energy was absorbed); ex: bond formation
62
Which reaction types are anabolic?
synthesis, endergonic
63
Which reaction types are catabolic?
decomposition, exergonic
64
Which reaction types are both anabolic and catabolic?
exchange, oxidation-reduction
65
Which reaction types are neither anabolic nor catabolic?
reversible
66
What is Collision Theory?
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
What is activation energy?
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
What are the 6 factors that can affect the rate of chemical reactions?
velocity, temperature, energy, size, concentration, and catalysts

A&P Unit 1 (5 decks)

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