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Anatomy and Physiology I > Ch.2 Intro to Chemistry > Flashcards

Ch.2 Intro to Chemistry Flashcards

1
Q

Matter

A

anything that has mass and occupies space

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2
Q

Weight

A

pull of gravity on mass

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3
Q

3 states of matter

A
  1. solid
  2. liquid
  3. gas
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4
Q

Solid

A

definite shape and volume

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5
Q

Liquid

A

changeable shape; definite volume

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6
Q

Gas

A

changeable shape and volume

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7
Q

Energy

A

capacity to do work or put matter into motion
Two forms of energy:
- Kinetic energy: energy in motion
- Potential energy: stored energy to be released

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8
Q

Forms of energy

A
  • Chemical
  • Electrical
  • Mechanical
  • Radiant (Electromagnetic)
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9
Q

Energy Conversions

A
  • Radiant energy can be converted to chemical
    energy
  • Chemical energy can be converted to mechanical
    energy
  • energy conversions are not 100% efficient – extra
    energy released as heat.
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10
Q

What elements make up 96.1% of living organisms?

A
  • Oxygen (O)
  • Carbon (C)
  • Hydrogen (H)
  • Nitrogen (N)
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11
Q

What elements make up 3.9% of living organisms?

A
  • Calcium (Ca)
  • Phosphorus (P)
  • Potassium (K)
  • Sulfur (S)
  • Sodium (Na)
  • Chlorine (Cl)
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12
Q

Protons

A
  • located in nucleus
    *1 Positive charge
    *1 amu
  • Number of protons = atomic number
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13
Q

Electrons

A
  • Orbit around nucleus
    – 1st orbit can hold up to 2 e-
    –2nd orbit can hold up to 8 e-
  • 1 negative charge
  • 0 amu
  • Number of electrons =
    number of protons
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14
Q

Neutrons

A
  • located in nucleus
  • No electrical charge
  • 1 amu
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15
Q

Atomic mass =

A

Number of protons + Number of neutrons

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16
Q

Atomic weight

A

average mass of all stable atoms for that element

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17
Q

Atomic number

A

number of protons

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18
Q

Atomic number - mass number =

A

number of neutrons

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19
Q

Atomic number - number of electrons =

A

electrical/ net charge of ion

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20
Q

an ion

A

an atom that has either gained or lost electron(s)

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21
Q

Isotopes

A
  • atoms of the same element
  • Ex: Iodine - same # of protons and electrons but different # of neutrons
  • can often be unstable (break down over time to release energy), used medically for diagnosis and harmful
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22
Q

How can isotopes be used medically for diagnosis?

A

Ex: radioactive iodine (Iodine 131, normal iodine-126) can be used to test for thyroid function

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23
Q

How can isotopes be harmful?

A

Radon gas results from decay of uranium in the ground, can cause cancer

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24
Q

molecule

A
  • two or more atoms bonded together (H2)
  • two or more of the same element bonded together (O2)
25
Q

Compound

A
  • two or more different kinds of atoms bonded together
  • Ex: (C6H12O6) Glucose, (H2O) Water, Salt (NaCl), Methane (CH4)
26
Q

Chemical bonds

A
  • forces that hold together atoms of a molecule or compound
  • bonding depends on the # of electrons in the outermost (valence) shell
27
Q

Octet Rule

A

stable if valence shell holds max number of electrons

28
Q

Types of Chemical Bonds

A
  1. ionic
  2. covalent
  3. hydrogen
29
Q

Ionic Bond

A

Electrons given away or accepted
- positive and negative charge

30
Q

Covalent Bond

A

Involve the sharing of electrons between atoms

31
Q

positive charge

A

more protons than electrons

32
Q

negative charge

A

more electrons than protons

33
Q

polar covalent

A

unequal sharing of electrons
- compounds tend to dissolve in water

34
Q

non polar covalent bond

A

equal sharing of electrons
- compounds tend to not dissolve in water

35
Q

Hydrogen bonds

A

form due to the polar covalent bonds of molecules
- Ex: hydrogen bonds between water molecules

36
Q

Inorganic compounds

A
  • water
  • salts
  • acids/ bases
37
Q

Organic compounds

A

macromolecules
contain carbon-hydrogen bonds
- proteins
- carbohydrates
- lipids
- nucleic acids

38
Q

Properties of water

A
  1. high heat capacity: requires high energy input in the form of heat to change temp
  2. high heat of vaporization: requires high energy input to change it from liquid to gas
  3. universal solvent: dissolves most molecules
  4. reactivity: in chemical reactions
  5. cushioning
  6. cohesion + surface tension
  7. Ice is lighter than water
  8. transparent: color less
39
Q

Salt

A
  • inorganic compound that dissolves in water and charged particles called electrolytes
    Ex: CaCO3 (calcium carbonate) –> Ca^2+ + CO3^2-
40
Q

Acid

A

substances that releases H+ (proton donor)

41
Q

Base

A

substances that take up H+ (proton acceptors) reduce the acidity of the solution
EX:
1. NaOH –> Na+ + OH-
2. OH- + H+ –> H2O

42
Q

Strong acids and bases

A

they are completely ionized (dissociates) in solution and can affect the pH of the solution

43
Q

pH scale

A
  • measures the amount of free H+ and free OH- in a solution
  • pH homeostasis is essential
  • 0-7 = acidic
  • 7-14 =basic
44
Q

Buffers

A
  • maintain pH
  • are weak acids and bases that donate or accept protons to help resist changes in pH, they do not completely dissociate
  • Ex: carbonic acid -bicarbonate system (blood)
45
Q

carbonic acid -bicarbonate system (blood)

A
  1. H2CO3 (carbonic acid = weak acid) –> HCO3- + H+ (bicarbonate + hydrogen ions)
    - Response: rise in pH –> becomes more basic –> compound dissociates
  2. HCO3- + H+ (bicarbonate + hydrogen ions) –> H2CO3 (carbonic acid = weak acid)
    - Response: drop in pH –> becomes more acidic
46
Q

Dehydration synthesis

A
  1. 2 monomers
  2. water is released –> removal of OH from one monomer and removal of H from the other monomer at the site of bond formation
  3. a covalent bond links 2 monomers into a macromolecule
    Ex: Glucose + Fructose –> Sucrose
47
Q

Hydrolysis

A
  1. Macromolecule linked by a covalent bond
  2. water is added –> monomers are released by adding OH to one monomer and H to the other monomer
  3. 2 monomers
    Ex: Sucrose –> Glucose + Fructose
48
Q

Carbohydrates (sugars)

A
  • polymer of monosaccharides
  • monosachraides: glucose and fructose
    function:
  • energy source: ATP
  • energy storage for animals: glycogen
  • energy storage for plants: cellulose
  • used for structure as proteoglycans
49
Q

Lipids

A
  • polymer of polysaccharides
  • molecules that are NOT soluble in water
  • 3 types: triglycerides, phospholipids, steroids
50
Q

Triglycerides

A
  • a type of lipid
    function:
  • energy storage
  • cushioning
  • insulation
  • good fats: unsaturated
  • bad fats: saturated
  • Ex: LDL (saturated) is bad cholesterol
51
Q

phospholipids

A
  • a type of lipids
    function:
  • form cell membranes
52
Q

Proteins

A
  • polymers of amino acids
    function:
  • structure
  • enzymes
  • contraction
  • immunity
  • regulation
  • carry oxygen
  • hormones
53
Q

Steroids

A
  • a type of lipids
    function
  • cell membranes
  • steroid hormones
  • vitamin D production
54
Q

Enzymes

A
  • not used up in reaction, speed up reaction and lowers energy of reaction
    1. Substrates bind at active sites –> enzyme changes to hold shape to hold substrates –> forms E-S complex
    2. internal rearrangements leading to catalysis occur
    – energy is absorbed –> bond is formed -> water is released
    3. product released –> enzyme returns to original shape and available to catalyze another reaction
55
Q

Nucleic acids

A
  • polymer of nucleotides
  • 2 types: DNA and RNA
56
Q

nucleotide

A

made up of phosphate, sugar and base
- make up nucleic acids

57
Q

ATP

A
  • a modified nucleotide
  • ATP –> ADP + P + Energy
58
Q

enzyme vs catalyst

A

enzyme:
- organic
- speeds up reaction by converting substrate into product
catalyst:
- inorganic
- increase or decrease the rate of a chemical reaction but remain unchanged

Anatomy and Physiology I (15 decks)

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