General Chemistry Ch. 1

Question 1

Atomic number =

Answer 1

of protons

Question 2

The mass of one proton is approximately _

Answer 2

1 amu

Question 3

Mass number =

Answer 3

of neutrons + # protons

Question 4

Which is larger: neutron or proton mass?

Answer 4

Neutron mass

Question 5

Define isotope

Answer 5

atoms with the same atomic number (# protons) but different mas number (# neutrons)

Question 6

The reactivity of an atom is determined by ___

Answer 6

Valence electrons

Question 7

Atomic mass ~~ __

Answer 7

Mass number

Question 8

List and describe the Hydrogen isotopes:

Answer 8

1H1 (Protium)
2H1 (Deuterium)
3H1 (Tritium)

Question 9

Define atomic weight

Answer 9

The weighted average of isotopes of that element

Question 10

Define Avogadro’s number

Answer 10

number of units in one mole of any substance (defined as its molecular weight in grams), equal to 6.02214076 × 10^23

Question 11

Define quanta

Answer 11

Energy emitted as electromagnetic radiation in discrete bundles

Question 12

Define Planck’s constant

Answer 12

Relates the energy in one quantum (photon) of electromagnetic radiation to the frequency of that radiation. 6.626176 x 10-34 joule-seconds

Question 13

The energy of an electron (decreases/increases) the farther out from the nucleus

Answer 13

Increases

Question 14

As electrons go from a lower energy to higher energy level, they get AHED. List the meaning of the acronym.

Answer 14

Absorb light
Higher potential
Excited
Distant from nucleus

Question 15

What is the speed of light in a vacuum?

Answer 15

3.00 x 10^8 m/s

Question 16

List the Hydrogen emission lines

Answer 16

1) Lyman series
2) Balmer series
3) Paschen series

Question 17

Describe the lyman series

Answer 17

Hydrogen spectral series of transitions and resulting ultraviolet emission lines of the hydrogen atom as an electron goes from n ≥ 2 to n = 1

Question 18

The (Lyman/Balmer) series has larger energy transitions

Answer 18

Lyman

Question 19

Describe the Balmer series

Answer 19

Series of spectral emission lines of the hydrogen atom that result from electron transitions from higher levels (n ≥ 3) down to the energy level with principal quantum number 2, resulting in four wavelengths emitted in the visible region

Question 20

Describe the Paschen series

Answer 20

A sequence of absorption or emission lines in the near-infrared part of the spectrum, due to hydrogen. They are caused by electron jumps in levels n ≥ 4 to n = 3

Question 21

Define the Heisenberg uncertainty principle

Answer 21

One can’t determine the exact momentum and position of an electron; either the momentum has to be stopped to determine position or the electron must be moving to determine momentum

Question 22

List and describe the 4 quantum numbers

Answer 22

The principal quantum number (n), the orbital angular momentum quantum number (l), the magnetic quantum number (ml), and the electron spin quantum number (ms).

Question 23

Define the Pauli exclusion principle

Answer 23

No 2 electrons in an atom can have same 4 quantum numbers

Question 24

What do quantum numbers describe?

Answer 24

The energy state of electrons

Question 25

A large principle quantum number (n) denotes ___

Answer 25

higher energy level and radius of electron shell

Question 26

Each shell can hold ___ electrons

Answer 26

2n^2

Question 27

The principle quantum number must be (positive/negative)

Answer 27

positive

Question 28

The angular momentum quantum number (l) determines the __

Answer 28

Shape and number of subshells within an energy level

Question 29

For angular momentum quantum number: if n = 1, l = ___

Answer 29

0

Question 30

What is the spectroscopic notation if l = 0?

Answer 30

s

Question 31

For angular momentum quantum number: if n = 2, l is ___

Answer 31

0 and 1

Question 32

For angular momentum quantum number: if n = 3, l = __

Answer 32

0, 1, and 2

Question 33

For angular momentum quantum number: if n = 4, l = ___

Answer 33

0, 1, 2, and 3

Question 34

What is the spectroscopic notation if l = 1?

Answer 34

p

Question 35

What is the spectroscopic notation if l = 2?

Answer 35

d

Question 36

What is the spectroscopic notation if l = 3?

Answer 36

f

Question 37

The maximum number of electrons that can be held within a subshell is determined by:

Answer 37

4l + 2

Question 38

The magnetic quantum number (ml_ describes ___

Answer 38

the specific particular orbital within a subshell where an electron is likely to be found

Question 39

Each orbital can hold __ electrons

Answer 39

2

Question 40

List the rule to determine magnetic quantum number

Answer 40

For l, ml = 2l + 1, with values between -l and +l

Question 41

If n = 1, ml is ___

Answer 41

0

Question 42

If n = 2, ml is ___

Answer 42

-1, 0, +1

Question 43

If n = 3, ml is ___

Answer 43

-2, -1, 0, +1, +2

Question 44

If n = 4, ml is ___

Answer 44

-3, -2, -1, 0, +1, +2, +3

Question 45

List the ml values of a s subshell

Answer 45

0

Question 46

List the ml values of a p subshell

Answer 46

-1, 0, +1

Question 47

List the ml values of a d subshell

Answer 47

-2, -1, 0, +1, +2

Question 48

List the ml values of an f subshell

Answer 48

-3, -2, -1, 0, +1, +2, +3

Question 49

Paired electrons are electrons in the (same/different) orbital with the (same/opposite) spins

Answer 49

same, opposite

Question 50

Electrons in different orbitals with the same ms values have __ spins

Answer 50

Parallel

Question 51

___ orbitals are spherical

Answer 51

s

Question 52

___ orbitals are dumbbell shaped

Answer 52

p

Question 53

Define the Aufbau principle

Answer 53

Electrons fill from lower to higher energy levels

Question 54

Define the n+l principle

Answer 54

If n+l are equal for 2 atoms, the subshell with the lower n value has lower energy and will fill with electrons first

Question 55

Define Hund's rule

Answer 55

In subshells with more than one orbital, the orbitals are filled so that there are a maximum number of half-filled orbitals with parallel spins

Question 56

For _ and _ subshells, electrons from lower energy subshells can give up electrons so that the higher energy subshells can be half-full instead of completely full

Answer 56

d and f

Question 57

Define paramagnetic

Answer 57

Materials with atoms of unpaired electrons that can orient their spins to align with magnetic field and will be weakly attracted to field

Question 58

Define diamagnetic

Answer 58

Materials where atoms have only paired electrons and will be slightly repelled by a magnetic field

Question 59

As n (the principal quantum number) increases, the radius and energy ____

Answer 59

Increase

Question 60

Protium has an atomic mass of _ and _ # of proton(s)

Answer 60

1 amu and 1 proton

Question 61

Deuterium has an atomic mass of __ and __# of protons and __ # of neutrons

Answer 61

2 amu; 1 proton, 1 neutron

Question 62

Tritium has an atomic mass of __ and __# of protons and __# of neutrons

Answer 62

3 amu; 1 proton, 2 neutrons

Question 63

__ is the weighted average of atomic isotopes

Answer 63

Atomic weight

Question 64

The energy of an electron ____ as n increases (as it goes farther from the nucleus)

Answer 64

Increases (becomes less engative)

Question 65

Define the Pauli Exclusion Principle

Answer 65

no two electrons of a given atom can have the same set of four quantum numbers

Question 66

The principal quantum number is _ and denotes _ and _

Answer 66

n; radius and energy level

Question 67

The azimuthal quantum number (angular momentum) is _ and denotes _ and _

Answer 67

l; shape and number of subshells

Question 68

The magnetic quantum number is __ and denotes __

Answer 68

ml; the particular orbital within a subshell where an electron is most likely to be found