Chapter 1 - Atoms

Question 1

Nuclide

Answer 1

A particular type of atom that possesses a characteristic atomic number (like Carbon-13).

Question 2

Z

Answer 2

Atomic number

Question 3

A

Answer 3

Mass number

Question 4

Monotopic elements

Answer 4

Occur naturally with only one nuclide (no isotopes).

Question 5

Allotrope

Answer 5

Different structural modifications of an element (graphite and diamond).

Question 6

Planck’s constant

Answer 6

h = 6.626 x 10^-34 Js

Question 7

SI unit of frequency

Answer 7

Hertz (Hz)

Question 8

E =

Answer 8

hc/wavelength

Question 9

Balmer series equation for hydrogen

Answer 9

v (wavelength) = R(1/4-1/n^2)

R = Rydberg constant = 1.07 x 10^7 m^-1

Question 10

angular momentum equation

Answer 10

mvr = n(h/2pi)

Question 11

Bohr radius of H

Answer 11

52.93 pm

Question 12

Wavefunction

Answer 12

The probability of finding an electron at a given point in space is determined from the function psi squared.

Question 13

Orbital quantum number

Answer 13

l (lowercase L) = n-1

Question 14

Orbital quantum number determines the

Answer 14

shape of the orbital.

Question 15

Magnetic quantum number

Answer 15

ml = between +l and -l

Question 16

Magnetic quantum number gives information about

Answer 16

the directionality of the atomic orbital.

Question 17

l values of s, p, d, f orbitals

Answer 17

s=0
p=1
d=2
f=3

Question 18

Degenerate

Answer 18

Orbitals that possess the same energy.

Question 19

Number of radial nodes

Answer 19

ns = n - 1
np = n - 2
nd = n - 3
nf = n - 4

Question 20

Zeff =

Answer 20

Zeff = Z - S

Question 21

Slater’s rules - electron in ns or np orbital

Answer 21

(i) ns, np electrons contribute S = 0.35
(ii) (n-1) electrons contribute S = 0.85
(iii) (n-2) electrons contribute S = 1.00

Question 22

Slater’s rules - electrons in nd or nf orbital

Answer 22

(i) nd, nf electrons contribute S = 0.35

(ii) electrons in any lower group contribute S = 1.00

Question 23

Typical elements

Answer 23

The first 2 elements of each main group (except group 18).

Question 24

Pnictogens

Answer 24

Group 15

Question 25

Chalcogens

Answer 25

Group 16

Question 26

Aufbau principle

Answer 26

Lowest energy orbitals are filled first.

Question 27

Hund’s rule

Answer 27

Electrons fill sublevels 1 at a time, with parallel spin, before pairing.

Question 28

Pauli exclusion principle

Answer 28

No two electrons in the same atom have the same set of n, l, ml, and ms quantum numbers.

Question 29

First ionization energy

Answer 29

For a gaseous atom, the internal energy change at 0 K associated with the removal of the first valence electron.

Question 30

Electron affinity

Answer 30

Minus the internal energy change at 0 K associated with the gain of one electron by a gaseous atom.