Chapter 1: Atomic Structure

Question 1

What is the charge of a proton?

Answer 1

+1e

Question 2

What is one atomic mass unit (amu)?

Answer 2

the approximate mass of one proton

Question 3

What is the atomic number (Z)?

Answer 3

number of protons in an atom

Question 4

How are elements identified/differentiated?

Answer 4

by their unique atomic number (the number of protons an atom of that element contains)

Question 5

What do each of the numbers represent?

Answer 5

Question 6

What is a neutrons charge?

Answer 6

zero / no charge

Question 7

How does a neutrons mass compare to that of a proton?

Answer 7

the mass is slightly larger than that of a proton

Question 8

The mass of an atom is made up almost entirely by the mass of _______.

Answer 8

the protons and neutrons within the nucleus

Question 9

What is the mass number (A)?

Answer 9

the sum of protons and neutrons

can vary within atoms of the same element

Question 10

Atomic weight

Answer 10

the weighted average of all isotopes of an element

Question 11

What are isotopes?

Answer 11

atoms of the same element with:

• same atomic number (protons)
• different mass number (neutrons)

Question 12

What doe the numbers represent in the following convention:

Answer 12

mass number = # protons + # neutrons

atomic number = # protons

Question 13

What are the numbers of protons and neutrons in these 3 carbon isotopes:

Answer 13

Question 14

Define electrons.

Answer 14

electrons move through the space surrounding the nucleus and are associated with varying levels of energy

Question 15

What is the charge of an electron?

Answer 15

– 1 e

Question 16

How does the mass of an electron compare to that of a proton?

Answer 16

that mass is approximately 1/2000 that of a proton

Question 17

What are energy levels of an electron?

Answer 17

an electrons energy level describes the distance at which an electron moves around the nucleus

Question 18

An electron closer to the nucleus will have a _______ energy level than one further from the nucleus.

Answer 18

lower

Question 19

Electrons further from the nucleus are called:

Answer 19

valence electrons

Question 20

What are 3 characteristics of valence electrons.

Answer 20

• most likely to become involved in bonds with other atoms because they experience the least electrostatic pull from their own nucleus
• determine the reactivity of an atom

Question 21

How does an atom become charged?

Answer 21

atoms can share or transfer their valence electrons to bonds allow the atom to increase its stability

Question 22

Cation vs anion?

Answer 22

Cation: positively charged atom

Anion: negatively charged atom

Question 23

Heisenerg uncertainty principle

Answer 23

we cannot know both the position and speed of a particle, (ex. electron) with perfect accuracy

the more we nail down the particle’s position, the less we know about its speed and vice versa

Question 24

Hund’s Rule

Answer 24

each orbital in a sublevel will receive 1 electron before any orbital receives 2

Question 25

Pauli Exclusion principle

Answer 25

1) no more than two electrons can occupy the same orbital
2) two electrons in the same orbital must have opposite spins

Question 26

principle quantum number

Answer 26

refers to the size and energy level of the orbital an electron is placed in

Question 27

azimuthal quantum number

Answer 27

3D shape of the orbital

Question 28

magnetic quantum number

Answer 28

orbital orientation

Question 29

ms quantum number

Answer 29

electron spin direction

Question 30

free radical

Answer 30

an atom or molecule with an unpaired electron