Atoms

Question 1

Atoms

Answer 1

Smallest unit of an element that retains said element’s chemical properties.

Question 2

What are the names and charges of the 3 subatomic particles?

Answer 2

Electrons- Negative
Protons- Positive
Neutrons- Neutral

Question 3

How can you figure out the number of energy levels an element has?

Answer 3

Use the periodic table.

Find the element, then look to the left at the number row your element is in. This tells you the number of electron orbitals the element’s atoms have.

Question 4

How do you create Bohr’s diagrams?

Answer 4

Center: Chem. Symbol, atomic #, # of neutrons

Surrounding middle: Electron orbitals.

Question 5

Halogens

Answer 5

Seventh column
Highly reactive
Will steal electrons from other atoms
Form ionic bonds
Fluorine, Chlorine, Bromine, Iodine, Astatine, Tennessine

Question 6

Alkali Metals

Answer 6

First column
Desperately wants to give away their singular valence electron
Form ionic bonds
Hydrogen, Lithium, Sodium, Potassium, Rubidium, Cesium, Francium

Question 7

Alkali Earth Metals

Answer 7

Second column
Give away their two valence electrons
Form ionic bonds
Beryllium, Magnesium, Calcium, Strontium, Barium, Radium

Question 8

Noble Gases

Answer 8

Eighth column
Full orbitals, chemically stable
Do not form bonds
Helium, Neon, Argon, Krypton, Xenon, Radon, Oganesson

Question 9

Isotopes

Answer 9

Different number of neutrons than usual

Question 10

Types of Orbitals

Answer 10

s: spherical, holds two electrons
p: three shapes, hold six electrons
d: five shapes, holds ten electrons
f: seven shapes, holds fourteen electrons

Question 11

Heisenberg Uncertainty Principle

Answer 11

We cannot measure the location and speed of an electron at the same time.

Question 12

Stable Atoms

Answer 12

Have full outer energy levels
 Level 1: 2e-
 Level 2: 8e-
 Level 3: 18e-, fine w/ 8
 Level 4: 32e-, fine w/ 8
 Level 5,6,7: 32e-, fine w/ 8