Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Chapter 10 modern atomic theory, and periodic table > Flashcards

Chapter 10 modern atomic theory, and periodic table Flashcards

1
Q

Protons and what are nearly equal in mass?

A

Neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

The mass number of an atom is the total of what?

A

Protons and neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Average atomic mass is the average mass of the what?

A

Isotopes of an element, and reflects the relative abundance of each isotope as it occurs in nature 

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Colors of the rainbow, abbrev
The visible portion of the spectrum is really what?

A

Roy G Biv 
All the colors of the rainbow combined

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the wave length?

A

Distance from crest of one wave to crest of the next

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the frequency?

A

The number of waves that pass a particular point each second

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the waves speed?

A

Distance a wave moves in a certain period of time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are photons

A

Energy bundles, or packets

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is Thompson’s plum putting model?

A

Electrons exist throughout the atom along with the positive particles (protons)
Thompson compared the particles in the atom to the dried fruits in plum pudding, randomly dispersed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is Neil Bohr’s planetary model?

A

Electrons are found at certain distances from the nucleus in allowable ENERGY LEVELS
Bohr believed electrons revolved around the nucleus in the same way as planets, orbit of the sun.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Bohr’s planetary model included what four things

A

One studied the line spectrum of hydrogen. Theorized each line corresponds to an energy transition for the electron in a hydrogen.
Two. When atoms absorb energy electrons move to higher energy levels -excited state.
Three LOWEST ENERGY STATEFOR A PARTICULAR ELECTION IS KNOWN AS GROUND STATE
Four When excited electrons return to ground state, they give off light of characteristic color, unique wavelength, and frequency as seen on emission spectra


How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is quanticized

A

Electron restricted to only certain allowed energies

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is ground state?

A

Bohrs lowest energy level

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is line spectrum?

A

Shows frequency of light energy emitted when electron has absorbed energy falls from higher energy level to lower energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is quanta?

A

Planck states energy never emitted in continuous stream, but only small, discreet packets quanta means how much

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the wave model work of the de Broglie and Schrodinger?

A

One it’s our current model of the atom
Two de Broglie proposed that we should treat electrons as waves as well as particles
Three  Schrodinger used math to calculate the probability or chance of finding an electron in a certain region outside the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is orbital?

A

Most probable location for an electron in electron cloud

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is principal energy level?

A

Most probable DISTANCE of electron from nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is sub level?

A

Division of principal energy level SPDF

20
Q

What is the principal quantum number?

A

Main energy level designation DISTANCE FROM THE NUCLEUS

21
Q

What is angular momentum quantum number?

A

It Depicts the energy sub level, the electron occupies

One the number of sub levels equals the principal quantum number
2- the energy level number one has one sub level energy number to has two sub level three energy level has three sublevels etc
We use letters for this - SPDF sublevels

22
Q

What is magnetic quantum number?

A

Depicts the ORIENTATION of a sub level in space
An s orbital has one position
a P orbital has three positions
D orbital has five positions
F orbital has seven positions

23
Q

What is aufbau principal

A

Electrons fill orbitals of lowest energy first

24
Q

What is Pauli exclusion principal

A

An orbital can only hold two electrons, and they must have a opposite spin

25
Q

What is Hunds rule?

A

When electrons fill orbitals of equal energy, one electron will occupy each orbital before they pair up 

26
Q

What are valence electrons?

A

Electrons in the outermost energy level

Highest occupied electrons in the outer, most energy level,

the group number matches this  (but not for transition metals!!)

27
Q

The principal quantum number, (main energy level) corresponds to the what?

A

Period Number for each element

28
Q

What is an octet

A

Eight valence electrons

29
Q

The number of valence electrons corresponds to what in the OLD SYSTEM
Locate Roman numerals.

A

The group number

30
Q

The table can be divided into four areas corresponding to what?

A

Which sub level is being filled by the last electrons

31
Q

What’s one way transition elements differ from others

A

They sometimes have exceptional configurations that are not as predicted

32
Q

There are never more than eight valence electrons

A
33
Q

Chapter 10 electromagnetic radiation is what?

A

Any form of energy that travels through space as a wave radio waves, microwaves, infrared, radiation, visible, light, UV radiation, x-rays, gamma rays

34
Q
Electromagnetic spectrum
A
35
Q

Today scientist describe light as what?

A

Both particles and waves. This is the dual nature of light explained by Einstein.

36
Q

When and excited electron returns to ground, state, energy is admitted as what

A

A photon is released. The color or a wavelength of the light is determined by the difference in energy between the two states, excited and ground.

37
Q

What are quantum numbers used to describe?

A

The location of electrons in an atom

38
Q

What is spin quantum number?

A

Defines if an electron spins clockwise or counterclockwise

39
Q

Describe this diagram

A
40
Q

N squared equals what?

A

The number of orbitals or O

41
Q

The Lewis structure equals what

A

Valence electrons only

42
Q
What element does this represent?
A

This is an electron configuration add the subscript numbers to figure out the element. This one is phosphorus.

43
Q

How do you draw the table using SPDF?
And what is it diagramming?

A

Top to bottom write one thru seven S
Then top to bottom starting at 2 write 2p
Then top to bottom starting at 3 write 3D
 Then, starting at four write 4F


44
Q

Explain the location of electrons

A

Electrons will be found in principal energy levels within the atom. Energy levels are designated as n
And is a positive integer and the first /lowest energy level is 1

Each energy level has sub levels.
Energy level ones (closest to nucleus) sub level level is 1s
Energy level twos sub level is 2S and 2p
Energy level threes sub level is 3S, 3P, 3D,
Energy levels 4 sub -level is 4s, 4p, 4d, 4F

The sub levels are like rooms on the floor of the building and hold room for orbitals

45
Q

Covalent compounds are a sharing of the valence electrons

A
46
Q

When diagramming orbital electrons start filling each group with the LEFT!

A

Chemistry (15 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions