Chapter 1

Question 1

Protons

Answer 1

• found in nucleus
• charge = 1.6*10^-19 OR +1
• Mass of 1 amu (atomic mass unit)
• Elements are defined by their # of protons

Question 2

The atomic number (Z) is equal to

Answer 2

the number of protons found in an atom of that element

Question 3

Neutrons

Answer 3

• Have no charge
• Found in nucleus with protons

Question 4

Mass number

Answer 4

Sum of protons and neutrons in nucleus

Question 5

Isotopes

Answer 5

• Share atomic # but different mass #s
• Only differ in number of neutrons, same amount of protons

Question 6

Electrons

Answer 6

• Found in orbitals around nucleus
• Charge of -1
• Electrons closer to nucleus have lower energy
• Electrons farther from nucleus (higher shells) have more energy

Question 7

Valence electrons

Answer 7

Electrons farthest from nucleus that have strongest interaction with surroundings and weakest interactions with nucleus
* Most likely to bond with other atoms due to weak pull from own nucleus
* Determine reactivity

Question 8

Losing electrons yields

Answer 8

positive charge

Question 9

Gaining electrons yields

Answer 9

negative charge

Question 10

Positively chargted atom

Answer 10

Cation

Question 11

Negatively charged atom

Answer 11

Anion

Question 12

Atomic Mass

Answer 12

Nearly equal to mass number (sum of protons and neutrons)
Think mass … mass number

Question 13

Atomic Weight

Answer 13

• Weighted average of all the different isotopes making up an element
• Number found on the periodic table
  Think weight … weighted average

Question 14

Mole

Answer 14

• Can be atoms, ions, molecules, etc.
• =6.02*10^23

Question 15

Planck Relation

Answer 15

Question 16

Planck’s constant

Answer 16

h=6.626*10^-34

Question 17

Angular Momentum

Answer 17

h = Planck’s constant
n = principal quantum number

Question 18

Energy of an electron

Answer 18

• Changes in discrete amounts with respect to the quantum number
• Energy of an electron increases (become less negative) the farther it is from the nucleus

R_H is the Rydberg unit of energy

Question 19

Ground State

Answer 19

• State of lowest energy
• All electrons are in lowest possible obirtals
• Desire this minimal energy state

Question 20

Excited State

Answer 20

• Electron is promoted to an orbit with a larger radius (higher energy)
• At least one electron has moved to a subshell with higher than normal energy
• Will occur due to extremely high temperatures or irradation

Question 21

Electron movement from low to high energy

Answer 21

AHED
A Absorb light
H Higher potential
E Excited
D Distant (from nucleus)

Question 22

Electromagnetic Energy of photons

Answer 22

Question 23

Line spectrum

Answer 23

Emission spectrum with each line corresponding to a specific electron transition

Question 24

Answer 24

Energy of emitted photon corresponds to difference in energy between the initial state (higher energy) and the final state (lower energy)
+E = emission
-E = absorption
To gain energy, must absorb energy from photons too jump up to higher energy level

Question 25

Maximum number of electrons within a shell

Answer 25

2n^2

Question 26

Principal Quantum Number (n)

Answer 26

* The larger the value of n, the higher the energy level and radius of the electron's shell * Difference in energy between two shells descreases as distance from nucleus increases

Question 27

Azimuthal (Angular Momentum) Quantum Number (l)

Answer 27

* Shape and number of subshells within a given principal energy level (shell) * l = 0 to (n-1)

Question 28

Subshells

Answer 28

l=0 (s) l=1 (p) l=2 (d) l=3 (f)

Question 29

Maximum number of electrons within a subshell

Answer 29

4l+2

Question 30

Magnetic quantum number (m_l)

Answer 30

* Specifies the orbital within a subshell where an electron will be most likely found at a certain time * Each orbital can hold max 2 electrons * Possible values: - l, 0, +l

Question 31

Orbital Shapes

Answer 31

Question 32

Subshell Amounts

Answer 32

S: 1 (2 elements) P: 3 (6 elements) D: 5 (10 elements) F: 7 (14 elements)

Question 33

Spin quantum number (m_s)

Answer 33

* When two electrons are in the same orbital, they must have opposite spins (AKA being paired) * Electrons in different orbitals with the same m_s have parallel spins

Question 34

____ will fill first

Answer 34

Subshells with lower energy

Question 35

n + l Rule

Answer 35

Lower n+l value has lower energy, therefore filling first

Question 36

Electron Configuration

Answer 36

Question 37

Electron Configuration of Ions

Answer 37

Will remove from subshell with higher principal quantum number first, then go down

Question 38

Half-filled and fully filled orbitals have ...

Answer 38

lower energy and higher stability

Question 39

TWO Electron Configuratoin Exceptions

Answer 39

Chromium: [Ar]4s^1 3d^5 * Half fills 3d subshell making a lot more stable Copper: [Ar] 4s^1 3d^10 * Fully fills 3d subshell making a lot more stable Other elements in this group exhibit the same behavior Similar shifts seen in f subshell but NEVER p subshell

Question 40

Paramagnetic

Answer 40

Materials made of atoms with unpaired electrons will orient their spins with the magnetic field, thus the material will be weakly attracted to the magnetic field

Question 41

Diamagnetic

Answer 41

Materials made of atoms with paried electrons, thus the material will be slightly repelled by a magnetic field

Question 42

Heisenberg Uncertainty Principle

Answer 42

It is impossible to determine at the same time with perfect accuracy the momentum and position of an electron

Question 43

Hund's Rule

Answer 43

Orbitals are filled so there are a maximum number of half-filled orbitals with parallel spins

Question 44

Parallel

Answer 44

Electrons in different orbitals with the same m_s

Question 45

Speed of light in a vacuum (C)

Answer 45

3*10^8