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test unit 4 Flashcards

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1
Q

John dalton model and what did

A

Billiard Ball Model
created Atomic Theory

all matter is made of atoms (T)
all atoms of an element are the same (f)
atoms of different elements are different (T)
chemical rxns involve rearranging atoms
elements combine in simple, whole-number ratios (F)

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2
Q

Atomic Theory

A

all matter is made of atoms (T)
all atoms of an element are the same (f)
atoms of different elements are different (T)
chemical rxns involve rearranging atoms
elements combine in simple, whole-number ratios (F)

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3
Q

Law of conservation of mass

A

if a system is closed, mass wont change

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4
Q

law of definite proportions

A

every compound has a set ratio (unique)

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5
Q

Law of multiple proportions

A

elements can combine in multiple ratios (ways)

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6
Q

Thomson experiment, what did, model

A

cathode ray experiment
discovers a mobile negative particle called the e-
plum pudding model (know model)
e- and positive dough

To test the properties of the particles, Thomson placed two oppositely-charged electric plates around the cathode ray. The cathode ray was deflected away from the negatively-charged electric plate and towards the positively-charged plate. This indicated that the cathode ray was composed of negatively-charged particles.

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7
Q

Rutherford model and what he do and experiment

A

discovers nucleus
positive core which contains the mass
atom is mostly empty space
gold foil experiment
KNOW MODEL
negative sphere outside of nucleus with squiggly lines
When he shot a beam of alpha particles at a sheet of gold foil, a few of the particles were deflected. He concluded that a tiny, dense nucleus was causing the deflections.

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8
Q

Group 1

A

Alkali Metals

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9
Q

Group 2

A

Alkaline Metals

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10
Q

Group 3-12

A

Transition Metals

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11
Q

Group 17

A

Halagens

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12
Q

Group 18

A

Noble Gases

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13
Q

isotope

A

same element, different mass, different number of neutrons, same number of protons

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14
Q

Schroedinger

A

mathematic model of the atom (based on probability)
a wave equation that accurately calculated the energy levels of electrons in atoms.
a bunch of dots (e- cloud, nucleus in middle)

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15
Q

Wavelength

A

the distance between 2 corresponding points on consecutive waves

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16
Q

Frequency

A

the number of waves per second

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17
Q

Electromagnetic radiation

A

anything that travels through space as a wave

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18
Q

Equation for frequency

A

=C/wavelength

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19
Q

Equation for C

A

wavelength times frequency

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20
Q

Equation for energy (E)

A

E=h times frequency
E = hc/wavelength

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21
Q

Pauli Exclusion Principal

A

no 2 e- can have the same set of quantum numbers

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22
Q

ion

A

same element, different charge (number of e-)

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23
Q

isoelectric

A

different elements, same number of e-

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24
Q

know how to do PEN stuff

A

knowWWWW

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25
Q

period

A

row

26
Q

group

A

column

27
Q

ionization energy

A

energy required to remove an e-

28
Q

ionization energy (period)

A

elements with a smaller atomic radius (more protons) have a higher IE
FACTORS: number of protons
effective nuclear charge (attracting e- closer to the nucleus)
coulombic force of attraction

29
Q

ionization energy (group)

A

elements with a smaller atomic radius (less energy levels) have a higher IE
FACTORS: number of energy levels
shielding effect
coulombic force of repulsion

30
Q

according to bohr’s model how many electrons are allowed for each energy level

A

1st: 2
2nd: 8
3rd: 18
4th: 32
5th: 50

31
Q

practice drawing Bohr’s model

A

DO IT

32
Q

noble gas configuration steps

A

find the element and determine the row
find noble gas in in row above
the difference in atomic number is the number of electrons left
always start with s sub level the first coeff is the row its in

33
Q

know orbital notation

A

practice

34
Q

hunds law

A

orbitals are 1/2 filled until all equal energy orbitals have a single e-

35
Q

know electron configuration chart

A

write it down

36
Q

sub level details

A

S: 2 e-, 1 orbital
P: 6 e-, 3 orbital
D: 10e-, 5 orbital
F: 14 e-, 7 orbital

37
Q

Does F or Li have a higher ionization energy

A

F has a higher ionization energy bc it has a smaller AR because it has a higher amount of protons. So, the nuclear charge is more effective. So, F has a stronger coulombic force of attraction, meaning its harder to remove the e-

38
Q

Does F or Li have a lower ionization energy

A

Li has a lower ionization energy bc it has a larger AR because it has a lower amount of protons. So, the nuclear charge is less effective. So, Li has a weaker coulombic force of attraction, meaning its easier to remove the e-

39
Q

Sb or N smaller ionization energy

A

Sb has a lower ionization energy bc it has a larger AR because it has amore energy levels, so there is a higher shielding effect. So, Sb has a greater coulombic force of repulsion, meaning the e- requires less energy to remove it

39
Q

Sb or N higher ionization energy

A

N has a higher ionization energy bc it has a smaller AR because it has less energy levels, so there is a lower shielding effect. So, N has a weaker coulombic force of repulsion, meaning the e- requires more energy to remove it

40
Q

understand how to find everages

A
41
Q

practice orbital notation

A

noble gas configuration

42
Q

how do metals fill valence levels

A

lose e- to fill

43
Q

how do non metals fill valence levels

A

gain e- to fill

44
Q

Planck

A

incandescent light bulbs
-energy is quantized (there are discrete packet of energy)
-metallic- continuous spectrum objects (rainbow)
-gaseous objects -line spectrum unique to each element

45
Q

explain how a mass spectrometer is used to determine the relative abundance of isotopes of an elemnet

A

The spectrometer ionizes atoms and molecules with a high energy e- beam and then deflects the ions through the magnetic field based on their mass to charge ratios

46
Q

what are valence e-

A

outermost e- used in bonding

47
Q

what is the octet rule

A

maximum valence e- is either 8 or 2

48
Q

how many valence e- do each of the main groups have

A

group 1: 1
group 2: 2
group 13: 3
group 14:4
15: 5
16: 6
17: 7
18: 8

49
Q

why are elements in the same column

A

have the same number of electrons in the outer orbital and are apart of the same chemical group

50
Q

why are elements in the same row

A

have the same number of valence electrons

51
Q

how to determine if atoms or elements are isoelectric to eachother

A

PEN!

52
Q

know pen

A

j know

53
Q

millikan experiment and what he did

A

discovered the mass and charge of electrons
oildrop experiment
measuring the force on oil droplets in a glass chamber between two electrodes, one above and one below. With the electrical field calculated, they could measure the droplet’s charge

54
Q

what did mosley do

A

discover nuclear charge, each element has a unique number of protons (atomic number)

55
Q

what did planck/einstein do

A

discovered energy is quantized

56
Q

what did chadwick do

A

discovers neutron
model is circle with dot in middle (nucleus whoch is p+ and n)
space is e- orbitting

57
Q

what did bohr do (know model) and experiment

A

discovered electrons are quantized (there are energy levels)

in hydrogen gas experiment,
electrons do not radiate energy as they orbit the nucleus, but exist in states of constant energy that he called stationary states.

58
Q

what did heinsberger do

A

you cannot know for certain the exact location and momentum of an atom

59
Q

what did pauli do

A

discovered no 2 e- can have the same set of quantum numbers

60
Q

what did hund do

A

discovered all orbitals are 1/2 filled until all equal energy orbitals have a single e- then can be doubly filled

61
Q

how to do specific heat and do practice problems

A

1) calculate the q for water using
-q=m deltaT C

2) Then use the answer for that as q (answer) then solve for metal and use same equation and solve for C

chemistry (10 decks)

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