Chapter 1-Atomic Structure

Question 1

Neutron

Answer 1

Located in nucleus.
Has no charge.
Mass around 1 amu.

Question 2

Electron

Answer 2

Located in shells circling nucleus.
Has a negative charge.
Mass is negligible.

Question 3

Atomic number

Answer 3

Number of protons given in the element.

Question 4

Mass number

Answer 4

Sum of elements protons and neutrons.

Question 5

Atomic mass

Answer 5

Is essentially equal to the mass number of the sum of elements protons and neutrons.

Question 6

Isotopes

Answer 6

Atoms of a given element that have the same atomic number(#protons), but different numbers of neutrons. Different mass numbers.

Question 7

Atomic weight

Answer 7

Weighted average of the different isotopes atomic mass of element isotopes.

Question 8

Rutherford postulation

Answer 8

An atom has a sense positively charged nucleus that makes up only a small fraction of the atom.

Question 9

Bohr model

Answer 9

A dense charged (proton) in the nucleus is surrounded by electrons revolving around orbits of distinct energy levels.

Question 10

Quantum

Answer 10

Energy differences between different energy levels. Described by Planck.

Question 11

Quantization

Answer 11

Not an infinite number of energy levels available to an electron. Electrons exists only at certain energy levels.

Question 12

Atomic absorption spectrum

Answer 12

Unique to an element.

Amount of energy absorbed for an electron to jump from a lower to a higher energy level.

Question 13

Atomic emission spectrum

Answer 13

Unique to an element.

Energy emitted in a photon when electron returns to ground state from an excited state.

Question 14

Quantum mechanical model

Answer 14

Points that electrons do not travel in defined orbits but rather are localized in orbitals.

Question 15

Heisenberg uncertainty principle

Answer 15

States that it is impossible to know both an electrons position and its momentum exactly at the same time.

Question 16

Quantum numbers

Answer 16

4 numbers: n, l, m(l), m(s)

Describe an electron in an atom.

Question 17

n

Answer 17

Principle number.

Describes the average energy of a shell.

Question 18

l

Answer 18

Azimuthal quantum number.

Describes sub shells within a given principle energy.

(s,p,d)

l= 0, (n-1)

Question 19

m(l)

Answer 19

Magnetic quantum number.

Specifies particular orbital within the sub she’ll.

Question 20

m(s)

Answer 20

Spin quantum number.

Indicates the spin orientation. (+- 1/2) of an electron in an orbital.

Question 21

n + l rule

Answer 21

Electrons fill the principal energy levels and subshells according to increasing energy.

Question 22

Hund’s rule

Answer 22

Sub shells with multiple orbitals Phil electron so that every orbital in the sub shell gets one electron before any of them gets a second.

Question 23

Paramagnetic

Answer 23

Materials of unpaired electrons that a line with magnetic fields attracting the material to the magnet.

Question 24

Diamagnetic

Answer 24

Materials have all paired electrons which cannot easily be realigned they are repelled by magnets.

Question 25

Valence electrons

Answer 25

Electrons in the outermost shell.

Available for interaction.

Question 26

Planck relation

Answer 26

E=hf

h=Plancks constant

Question 27

Angular momentum of electron

Answer 27

L=nh/2pie

Question 28

Energy of an electron (Bohr)

Answer 28

E=-R(H)/n^2

Question 29

Maximum electrons in a shell

Answer 29

2n^2

Question 30

Maximum electrons in a subshell

Answer 30

4l + 2

Question 31

Proton

Answer 31

Located in nucleus.
Has a positive charge.
Mass around 1 amu.