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dynamics of health > chem midterm > Flashcards

chem midterm Flashcards

1
Q

Different substances evenly mixed ex: sugar water, salt water

A

Homogenous mixture

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2
Q

Different substances not evenly mixed ex: trail mix, cereal

A

heterogeneous mixture

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3
Q

The digits that carry meaning and contribute to its precision

A

Significant figures.

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4
Q

The measure of how much mass is in a given volume

A

density

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5
Q

Amount of matter an object contains

A

mass

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6
Q

spaced occupied by a 3 dimensional shape

A

volume

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7
Q

the average mass of an atom of an element (measured in AMU)

A

Atomic mass

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8
Q

The # of protons in the nucleus of an atom of that element

A

Atomic number

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9
Q

Different forms of an element might have the same number of protons but a different number of neutrons (These variations result in a different atomic mass)

A

Isotope

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10
Q

An atom or group of bonded atoms that has a positive charge (cation) or negative charge (anion)

A

Ion

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11
Q

of protons and neutrons in the nucleus

A

Mass number

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12
Q

The spontaneous emission of radiation from the nucleus of an unstable atom

A

Radioactivity

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13
Q

The time it takes for half of the atoms in a sample to undergo radioactivity decay

A

half-life

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14
Q

The amount of a substance that contains as many particles as there are atoms in exactly 12 g or carbon 12

A

Mole

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15
Q

A form of energy that exhibits wave-like behaviors as it travels through space

A

electromagnetic radiation

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16
Q

The lowest state of an atom

A

ground state

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17
Q

A state in which an atom has a higher potential energy than its ground state

A

Excited state

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18
Q

(lambda) the distance from crest to crest

A

wavelength

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19
Q

(Nu) the number of waves that pass a given point on a specific time– usually one second (waves per second)

A

frequency

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20
Q

A particle of electromagnetic radiation (ER) having no mass and carrying a quantum (fixed amount) of energy

A

Photon

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21
Q

a single packet of matter or energy

A

quantum

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22
Q

a three-dimensional region around the nucelus that indicates the probable location of an electron.

A

orbital

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23
Q

arrangement of electrons in an atom or ion. Describes how electrons ocupy different sublevels or orbitals.

A

electron configuration

24
Q

Electrons are arranged in an atom such that each electron occupies the lowest energy orbital available

A

Aufbau principle

25
Q

Electrons should be placed into separate orbitals before going to the same orbitals

A

Hund’s rule

26
Q

Two arrows cant go on the same orbital

A

Pauli exclusion

27
Q

Electronegativity increases across a….

A

period

28
Q

Energy decreases down a…

A

group

29
Q

negatively charged ion

A

anion

30
Q

postively charged ion

A

cation

31
Q

metal

A

good conductors of heat and electricity

32
Q

the chemical bonding that results from the electrical attraction between laerge number of cations and anions that have been created by the transfer of electrons.

A

ionic bond

33
Q

properties opposite to metals, made from ions

A

non-metal

34
Q

substances that conduct electricity when dissolved in water or melted

A

electrolytes

35
Q

elements that have properties intermediate between metals and non-metals

A

metalloid (semi-metal)

36
Q

highly reactive, first row of periodic table

A

alkali metals

37
Q

Alkaline earth metals

A

second row of the periodic table

38
Q

group 17 of the periodic table, highly reactive and tend to form compouds by gaining electrons from other elements

A

halogen

39
Q

group 18, low reactivity, full outer electron shell, stable

A

noble gases

40
Q

one half the distance between the nuclei of identical atoms that are bound together

A

atomic radius

41
Q

a measure of the ability of an atom in a compound to atraxct the valence elections of another atom in that compound on isolated atoms

A

electronegativity

42
Q

the energy required to remove one electron from a neutral atom of an element (measured in the gas phase)

A

ionization energy

43
Q

the electrons occupying the atoms highest energy level (they are always in the S and P orbitals)

A

Valence electrons

44
Q

Why do certain elements emit radioactivity?

A

An unfavorable ratio of neutrons to protons can yeild an unstable atom emitting radioactivity (particles/energy) make the atom more stable.

45
Q

What are the forms of radioactive decay?

A

Alpha, Beta, Gamma

46
Q

what happens when an element emits alpha radiation?

A

4/2He: subtract 4 from the top number and 2 from the bottom number

47
Q

what happens when an element emits beta radiation?

A

0/-1e: add 1 to the bottom number

48
Q

Kilo- (King)

A

1,000

49
Q

Hecto-(henry)

A

100

50
Q

Deka-(died)

A

10

51
Q

Deci-(drinking)

A

1/10

52
Q

centi-(chocolate)

A

1/100

53
Q

milli-(milk)

A

1/1000

54
Q

Micro-

A

1/1000000

55
Q

What happens to an electron in an atom if it aborbs a quantym of energy? What happens when it loses energy?

A

An electron that abosrbs a quantum of energy will jump to an excited state and when it loses energy it decays and drops down to a ground state.

56
Q

What is a valence electron? How can you determine the # of valence electrons for any given element?

A

valence electrons are the electrons with the most energy. They are the furthest electrons from the nucelus and are responsible fo rthe characterisitifcs of that element. The number of valence elections for the main block elemernts (those elements in the s + p blocks) is found from the group number: group 1=1, group 2=2, group 13=3, group 14=4, group 15=5, group 16=6, group 17=7 ground 18=8.

57
Q

Which groups of elements are the most reactive?

A

group 1, the alkali metals and group 17, the halogens

dynamics of health (21 decks)

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