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GB1 > GB1: Chapter 2 > Flashcards

GB1: Chapter 2 Flashcards

1
Q

Atomic nucleus

A

protons and neutrons packed tightly at center of atom, is + charged due to protons

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2
Q

common elements of human body

A

carbon, nitrogen, hydrogen, oxygen, potassium, phosphorus, magnesium, calcium, chlorine, sodium, sulfur

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3
Q

compound

A

2 or more elements combined in fixed ratio

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4
Q

electron cloud

A

electrons rapidly move about the nucleus, forming a cloud of - charge

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5
Q

Electron orbitals

A

3D space where electron is found 90% of the time
No more than 2 electrons occupy single orbital

In 2nd energy shell, 4 orbitals can hold up to 8 electrons (2s & 2p = 8 electron spaces)

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6
Q

electron shell

A

fixed energy shell, electron’s state of potential energy

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7
Q

electrons absorb/gain energy:
electrons lose energy:
the amount of energy gained/lost:

A

increase in energy level (further away from nucleus)

decrease in energy level (closer to nucleus)

equals the amount of energy between shells

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8
Q

elements

A

pure substances, cannot be broken down into other substances

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9
Q

energy

A

capacity to cause change

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10
Q

every electron shell has electrons at certain energy level that are distributed among…?

A

specific number of orbitals of certain size and orientation

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11
Q

how does atom stay together?

A

attraction between the +charged nucleus and -charged electrons

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12
Q

in chemical rxns, what is involved?

A

valence electrons are directly involved, chemical bonds are being broken/formed

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13
Q

inert elements

A

chemically nonreactive elements that have complete valence shell

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14
Q

matter

A

anything that has mass and takes up space, made up of elements

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15
Q

molecules

A

2 or more atoms covalently bonded together

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16
Q

potential energy

A

energy that matter has due to its location or structure, energy locked into structure-not currently changing
matter naturally moves toward the lowest possible state of potential energy (nelsen’s law #2!)

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17
Q

subatomic particles

A

these make up an atom
proton +
neutron no charge
electron -

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18
Q

trace elements w/ example

A

elements required by organisms in minute quantities (less than 0.01% mass) ex: fluorine, boron

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19
Q

valence shell, what does it determine?

A

outermost shell of electron, it determines the chemical behavior of atom

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20
Q

atomic number

A

of protons

of protons = # of electrons in neutral atom

21
Q

Atomic mass (3)

A

atom’s total mass, weighted average of isotopes, can be estimated by mass number (# protons + # neutrons)

change in proton # = different element
change in neutron # = isotope of element

unit of measurement is DALTONS

22
Q

isotopes

A

Atoms of element that have different number of neutrons (different atomic masses)

23
Q

radioactive isotopes

A

nucleus decays spontaneously and gives off particles and energy. unstable, so goes to lowest energy level for stability - nelsen’s law #2!
when this changes the # of protons, atom changes to different element

Parent isotope decays into its daughter isotope at fixed rate

24
Q

radioactive tracers

A

diagnostic tools in medicine: radioactive isotopes are incorporated into biologically active molecules used as tracers to track atoms during metabolism
also used with sophisticated imaging instruments

25
Q

half-life

A

time it takes for 50% of parent isotope to decay

26
Q

radiometric dating

A

process to measure ratio of different isotopes and calculate how many half lives have passed since organism was fossilized/rock was formed

27
Q

chemical bonds w/ 5 types

A

attraction between atoms with incomplete valence shells through transfer or sharing of electron(s)

single, double, triple: increase in bond # = decrease in bond length = more energy in bonds

van der waals
hydrogen bonds
ionic bonds
polar covalent bonds
nonpolar covalent bonds

28
Q

bonding capacity

A

atom’s valence, maximum # of bonds that atom can form with other atoms to complete octet, corresponds to # of electrons needed to complete valence shell octet

29
Q

covalent bond

A

the sharing of a pair of electrons between 2 atoms

30
Q

nonpolar covalent bonds

A

EQUAL sharing of pair of electrons between 2 atoms due to relatively equal values in electronegativity

31
Q

polar covalent bonds

A

UNEQUAL sharing of pair of electrons between 2 atoms due to large difference in electronegativity, resulting in partial charges (more EN, negative partial charge; less EN, positive partial charge)

32
Q

electronegativity

A

attraction of particular atom for electron in covalent bond
more EN = stronger pull of electrons

33
Q

ionic bonds

A

bond formation due to ATTRACTION between cation (+charged ion) and anion (-charged ion) because of complete transfer of valence electron(s) from one atom to another (this is due to the extremely great difference in electronegativity)
compounds formed: salts, ionic compounds in 3D lattice

34
Q

hydrogen bonds

A

weaker chemical interaction, hydrogen atom that is covalently bonded to an electronegative atom (giving it partially +charge) is ALSO ATTRACTED to another electronegative atom (with partial -charge)

in cells, usually to oxygen or nitrogen

35
Q

chemical behavior of atom

A

determined by distribution of electrons in shells, especially in outer shell
atoms with same number of valence shells exhibit similar chemical behaviors

36
Q

van der waals interactions

A

weakest interaction; only occurs when atoms and molecules are close together, due to the partially negative positive and negative parts of atom/molecule as electrons aren’t always evenly distributed

37
Q

molecular shape

A

depends on position of atom’s orbitals.
size/shape are what determine molecule’s function and how they interact with each other

38
Q

hybridization

A

when atom forms COVALENT BONDS, the orbitals in its valence shell undergo rearrangement
1s + 3p of valence shell in covalent bond = 4 hybrid orbitals in teardrop shapes

39
Q

morphine vs endorphine

A

have similar effects due to similar molecular structures as they bind to same receptor in brain

40
Q

chemical equilibrium

A

DYNAMIC EQUILIBRIUM
forward/reverse rxns occur at same rate, relative concentrations of reactant/product don’t change

more reactant-> produce more products
More product -> produce more reactants

41
Q

orbitals, electron configuration

A

electrons occupy opposite regions of atom (because they repel each other)
electron spins must be opposite of each other
electron configuration shows how electrons are distributed in orbitals

42
Q

reactivity of atom

A

due to the unpaired electrons in one or more orbitals in valence shell

43
Q

1s___

A

1s = orbital
1 = energy shell
s = determines orbital’s shape

s = sphere
p = propellor

44
Q

chemical reactions

A

forming/breaking chemical bonds leading to change in composition of matter
all are theoretically reversible

45
Q

polar covalent bond value

A

0.4 < EN < 0.7

46
Q

nonpolar covalent bond value

A

EN < 0.4

47
Q

ionic bond value

A

EN > 1.7

48
Q
A

GB1 (11 decks)

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