Atomic Structure Flashcards

1
Q

Isotopes

A

Atoms of the same element that differ in mass due to a different number of neutrons

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

John Dalton’s 4 Findings

A
  • All atoms are composed of indivisible atoms
  • All atoms of a given atom must be identical in every way
  • Atoms of different elements must be different in some fundamental way
  • Compounds are produced from a reaction between different atoms (elements)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Rutherford’s Experiment - 2 Observations

A

1) Most of the alpha particles passed through the gold foil
2) A few particles were deflected or back-scattered

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

Rutherford’s Experiment - 2 Conclusions

A

1) Most of the an atom is empty space
2) An atom contains a dense core with a positive charge

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

Proton

A

Location: Nucleus
Charge: +1
Mass: 1

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

Neutron

A

Location: Nucleus
Charge: 0
Mass: 1

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

Electron

A

Location: In orbitals outside the nucleus
Charge: -1
Mass: 0

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

Alpha particle

A

A charged helium nucleus

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

Beta particle

A

A high speed electron

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

Atomic number

A

The number of protons in an atom

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

Why is an atom electrically neutral?

A

The number of protons is equal to the number of electrons in an atom

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

Every element has a unique _____

A

Atomic number

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

Mass number

A

The number of protons plus the number of neutrons

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

Label parts: 11 5 B

A

Mass number: 11
Protons: 5
Atomic number: 5
Electrons: 5
Neutrons: 6
Word form: Boron - 11

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

Atomic mass

A

The weighted average of all naturally occurring isotopes of an element (decimal number)

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

How is the atomic mass of an element determined?

A
  • Convert the percent abundances to a decimal (move decimal point two places to the left)
  • Multiply the mass number by the converted percent abundance
  • Add all the products
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

2 facts about atomic mass

A

1) Should be somewhere between the two original masses
2) Should be closest to the mass of the most abundant isotope

18
Q

Bohr model description

A

Electrons revolve around the nucleus in one of seven shells or rings called potential energy levels (PELS). The rings correspond to rows or periods of the periodic table.

19
Q

Compare the energy of electrons closest to the nucleus to the energy of electrons farthest from the nucleus

A

Close to nucleus = lowest energy
Farthest from nucleus = highest energy

20
Q

What is the maximum number of electrons each PEL can hold?

A

1 - 2 electrons
2 - 8 electrons
3 - 18 electrons
4 to 7 - 32 electrons

21
Q

What is the shortcoming of the Bohr model?

A

It is only a 2-D representation

22
Q

Valence electrons

A

Electrons in the outermost PEL

23
Q

Noble gases (group 18)

A

Odorless, colorless, nonflammable gases that are inert due to a complete octet

24
Q

Inert

A

Do not react

25
If an ion is positively charged, it…
Lost electrons
26
If an ion is negatively charged, it…
Gained electrons
27
Isoelectronic
Have the same electronic configuration
28
Ground state electronic configuration
- Normal condition - Electrons are in the lowest PELS - Fill lower energy PEL first
29
Excited state electronic configuration
- Condition when an atom is bombarded by energy - Electrons shift from low energy PELS to high energy PELS
30
How is the color produced from a Ne light?
Electrons shift from a high energy state to a lower energy state and release energy in the form of visible light
31
Line spectra
Produced from events and each element has a unique line spectra
32
Spectra/spectrum
A series of colors which forms when light is refracted
33
Spectroscope
A device that shows the component colors in a beam of light
34
Electromagnetic spectrum
Longest waves/lowest energy to shortest waves/highest energy: radio waves, microwaves, infrared, visible light, UV light, x-rays, gamma rays
35
Wave mechanical model
- Modern model of an atom - Helps us locate where an electron is
36
Orbital
A region of space or volume where there is a high probability of finding an electron
37
Wave mechanical model chart
PEL - sublevel - number of orbitals - max number of electrons 1 - 1s - 1 orbital - 2 electrons 2 - 2s, 2p - 1 orbital + 3 orbitals = 4 orbitals - 2 electrons + 6 electrons = 8 electrons 3 - 3s, 3p, 3d - 1 orbital + 3 orbitals + 5 orbitals = 9 orbitals - 2 electrons + 6 electrons + 10 electrons = 18 electrons 4 - 4s, 4p, 4d, 4f - 1 orbital + 3 orbitals + 5 orbitals + 7 orbitals = 16 orbitals - 2 electrons + 6 electrons + 10 electrons + 14 electrons = 32 electrons
38
Hund’s Rule
Keep the electrons in separate orbital boxes first, then start to double them up
39
Lewis electron dot diagrams
Show the valence electrons that are lost, gained, or shared when forming a bond only
40
What characteristic allows elements in a group to share similar chemical properties?
Same number of valence electrons