Atomic Structure

Question 1

Isotopes

Answer 1

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

Question 2

John Dalton’s 4 Findings

Answer 2

• 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)

Question 3

Rutherford’s Experiment - 2 Observations

Answer 3

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

Question 4

Rutherford’s Experiment - 2 Conclusions

Answer 4

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

Question 5

Proton

Answer 5

Location: Nucleus
Charge: +1
Mass: 1

Question 6

Neutron

Answer 6

Location: Nucleus
Charge: 0
Mass: 1

Question 7

Electron

Answer 7

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

Question 8

Alpha particle

Answer 8

A charged helium nucleus

Question 9

Beta particle

Answer 9

A high speed electron

Question 10

Atomic number

Answer 10

The number of protons in an atom

Question 11

Why is an atom electrically neutral?

Answer 11

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

Question 12

Every element has a unique _____

Answer 12

Atomic number

Question 13

Mass number

Answer 13

The number of protons plus the number of neutrons

Question 14

Label parts: 11 5 B

Answer 14

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

Question 15

Atomic mass

Answer 15

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

Question 16

How is the atomic mass of an element determined?

Answer 16

• 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

Question 17

2 facts about atomic mass

Answer 17

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

Question 18

Bohr model description

Answer 18

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.

Question 19

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

Answer 19

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

Question 20

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

Answer 20

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

Question 21

What is the shortcoming of the Bohr model?

Answer 21

It is only a 2-D representation

Question 22

Valence electrons

Answer 22

Electrons in the outermost PEL

Question 23

Noble gases (group 18)

Answer 23

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

Question 24

Inert

Answer 24

Do not react

Question 25

If an ion is positively charged, it…

Answer 25

Lost electrons

Question 26

If an ion is negatively charged, it…

Answer 26

Gained electrons

Question 27

Isoelectronic

Answer 27

Have the same electronic configuration

Question 28

Ground state electronic configuration

Answer 28

• Normal condition
• Electrons are in the lowest PELS
• Fill lower energy PEL first

Question 29

Excited state electronic configuration

Answer 29

• Condition when an atom is bombarded by energy
• Electrons shift from low energy PELS to high energy PELS

Question 30

How is the color produced from a Ne light?

Answer 30

Electrons shift from a high energy state to a lower energy state and release energy in the form of visible light

Question 31

Line spectra

Answer 31

Produced from events and each element has a unique line spectra

Question 32

Spectra/spectrum

Answer 32

A series of colors which forms when light is refracted

Question 33

Spectroscope

Answer 33

A device that shows the component colors in a beam of light

Question 34

Electromagnetic spectrum

Answer 34

Longest waves/lowest energy to shortest waves/highest energy: radio waves, microwaves, infrared, visible light, UV light, x-rays, gamma rays

Question 35

Wave mechanical model

Answer 35

• Modern model of an atom
• Helps us locate where an electron is

Question 36

Orbital

Answer 36

A region of space or volume where there is a high probability of finding an electron

Question 37

Wave mechanical model chart

Answer 37

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

Question 38

Hund’s Rule

Answer 38

Keep the electrons in separate orbital boxes first, then start to double them up

Question 39

Lewis electron dot diagrams

Answer 39

Show the valence electrons that are lost, gained, or shared when forming a bond only

Question 40

What characteristic allows elements in a group to share similar chemical properties?

Answer 40

Same number of valence electrons