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test unit 4 Flashcards

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
period
row
26
group
column
27
ionization energy
energy required to remove an e-
28
ionization energy (period)
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
ionization energy (group)
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
according to bohr's model how many electrons are allowed for each energy level
1st: 2 2nd: 8 3rd: 18 4th: 32 5th: 50
31
practice drawing Bohr's model
DO IT
32
noble gas configuration steps
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
know orbital notation
practice
34
hunds law
orbitals are 1/2 filled until all equal energy orbitals have a single e-
35
know electron configuration chart
write it down
36
sub level details
S: 2 e-, 1 orbital P: 6 e-, 3 orbital D: 10e-, 5 orbital F: 14 e-, 7 orbital
37
Does F or Li have a higher ionization energy
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
Does F or Li have a lower ionization energy
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
Sb or N smaller ionization energy
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
Sb or N higher ionization energy
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
understand how to find everages
41
practice orbital notation
noble gas configuration
42
how do metals fill valence levels
lose e- to fill
43
how do non metals fill valence levels
gain e- to fill
44
Planck
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
explain how a mass spectrometer is used to determine the relative abundance of isotopes of an elemnet
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
what are valence e-
outermost e- used in bonding
47
what is the octet rule
maximum valence e- is either 8 or 2
48
how many valence e- do each of the main groups have
group 1: 1 group 2: 2 group 13: 3 group 14:4 15: 5 16: 6 17: 7 18: 8
49
why are elements in the same column
have the same number of electrons in the outer orbital and are apart of the same chemical group
50
why are elements in the same row
have the same number of valence electrons
51
how to determine if atoms or elements are isoelectric to eachother
PEN!
52
know pen
j know
53
millikan experiment and what he did
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
what did mosley do
discover nuclear charge, each element has a unique number of protons (atomic number)
55
what did planck/einstein do
discovered energy is quantized
56
what did chadwick do
discovers neutron model is circle with dot in middle (nucleus whoch is p+ and n) space is e- orbitting
57
what did bohr do (know model) and experiment
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
what did heinsberger do
you cannot know for certain the exact location and momentum of an atom
59
what did pauli do
discovered no 2 e- can have the same set of quantum numbers
60
what did hund do
discovered all orbitals are 1/2 filled until all equal energy orbitals have a single e- then can be doubly filled
61
how to do specific heat and do practice problems
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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