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Chemistry > Unit 2 Test > Flashcards

Unit 2 Test Flashcards

1
Q

what are 3 subatomic particles and what does each one do

A

protons: determine identity of an element
neutrons: hold nucleus together and influence mass
electrons: determine the chemical properties of an element

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2
Q

how do their masses compare (according to 1)

A 
protons/neutrons= same mass (1.67 x 10^-24)
electrons= (9.11 x 10^-28)
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3
Q

how do electrons emit light?

A

when an electron moves from a high to a low energy level it results in a burst of light

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4
Q

how many electrons can be held in the third principal energy level

A

18

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5
Q

how many sublevels are in the 2nd principal level

A

2

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6
Q

how are the elements arranged on the modern periodic table

A

increasing atomic number

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7
Q

how many neutrons doe Rn-226 have?

A

140

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8
Q

How does an isotope differentiate from a neutral atom?

A

Isotopes have the same # of protons but a different # of neutrons.
(also all have different mass numbers)

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9
Q

Where are neutral atoms found?

A

periodic table

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10
Q

Difference between atomic mass and mass number? what do each represent?

A

atomic mass: weighted average mass of atoms in a naturally occurring sample of the element, reflects both the mass and relative abundance.
mass number: # of protons + neutrons

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11
Q

what is the stability of an isotope based on?

A

ratio of neutrons to protons

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12
Q

which type of nuclear emission is the most similar to high x-rays?

A

gamma

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13
Q

how does the atomic emission spectrum compare to the visible spectrum

A

visible spectrum: only small chunk (rainbow colors)

atomic emission: everything

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14
Q

what determines a element’s chemical properties?

A

electrons

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15
Q

how do elements configuration relate to their position on the periodic table

A

they show the amount of electrons (atomic number) and where they are located

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16
Q

whats the difference between an ion and a neutral atom

A

Ion has a different number of protons/electrons

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17
Q

describe modern atomic theory

A

electrons exist in a cloud

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18
Q

difference between physical and chemical change

A

chemical: change that produces matter with a different composition than the original matter
physical: some properties of a material change but the composition of the material does not change

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19
Q

signs of a chemical change

A
  • forms a precipitate
  • release of energy
  • bubbles
  • change of color
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20
Q

what types of substances cant be broken down by chemical processes

A

elements

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21
Q

differences and definitions of the different types of decay

A 
alpha:
-nucleus ejects 2 protons and neutrons simultaneously
-atomic # down 2
-atomic weight down 4
beta:
-neutron splits into proton and electron
-atomic # up 1
-atomic weight = no change
gamma:
-no change, just emits radiation (deadly)
22
Q

what is a half-life?

A

the time required for one-half of the nuclei of a radioisotope sample to decay to products

23
Q

how much of a 1000g sample would be left after 4 half-lives?

A

500>250>125>(62.5)

24
Q

what do the symbols represent in the equation:

c=(upside down)Yv

A

C= speed of light (m/s)
(upside down) Y= wavelength (m/s)
v= frequency (sec^-1)

25
Q

what do the symbols represent in the equation:

E=hv

A 
E= energy (joules)
h= Planck's Constant (J*sec)
v= frequency (hertz or sec^-1)
26
Q

what is atomic number

A

of electrons/protons

27
Q

what do the symbols represent in the equation:

a/zC

A 
a= protons + neutrons (mass number)
z= protons
c= element name
28
Q

what are two ways to write isotopes?

A

element name- mass number

mass #/protons x element name

29
Q

what are the two types of isotopes

A

stable: nucleus stays intact
unstable: nucleus decays and emits radiation

30
Q

define fission and fusion

A

fission: when atom divides into smaller parts
(EX: nuclear energy, bomb)
fusion: when 2+ atoms fuse together to become one
(EX: stars, new elements)

31
Q

strengths of the 3 types of decay?

A

alpha: encounter everyday
beta: skin protects us from it
gamma: goes through everything

32
Q

define atomic orbitals

A

space around the nucleus where the electrons exists

33
Q

each principal energy level surround the nucleus has a _________

A

specific # of sublvls within it

34
Q

each sublvl has a specific _______

A

shape & is designated by a letter

35
Q

each sublvl can only hold a certain ________

A

of electrons

36
Q

define aufbau principle

A

electrons fill the lowest energy lvls first

37
Q

define pauli explusion principle

A

only 2 electrons can share an orbital and they have opposite spin

38
Q

define hunds rule

A

electrons spread out of their last orbital

39
Q

define light

A

a stream of photons (packets of energy)

40
Q

what do different colors indicate

A

different wavelengths

41
Q

what is white a combination of

A

all the colors (light reflects color)

42
Q

different wave lengths carry different ________

A

amounts of energy

43
Q

first step:

A

receive energy and become excited

44
Q

when electrons get excited:

A

they absorb energy and move up an orbital from their ground state

45
Q

when they return to their ground state:

A

the energy is released in the forms of light. The color of the light depends on how much color it has

46
Q

define amplitude, wavelength and frequency

A

amplitude: waves height from bottom to top
wavelength: distance between crests (tops) of wave
frequency: # of wave cycles to pass a given point

47
Q

define quantum

A

amount of energy to move lvls

48
Q

define electron configurations

A

way electrons are arranged in various orbitals around nuclei

49
Q

wavelength and frequency are:

A

inversely proportional

50
Q

what is red on the visible spectrum

A

longest wavelength, lowest frequency

Chemistry (9 decks)

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