Chapter 7 Quantum Mechanics P2

Question 1

Electron Configuration

Answer 1

A representation of how electrons occupy orbitals in which orbitals are
represented as text and the number of electrons in each orbital is specified as a superscript

Question 2

Aufbau Principle

Answer 2

Electrons fill the lowest energy orbitals first

Question 3

Noble Gas Abbreviation

Answer 3

A method for abbreviating electron configurations and orbital diagrams. The
previous noble gas is given in brackets, and only electrons that are not part of the previous noble gas are
shown

Question 4

Orbital Diagram

Answer 4

A representation of how electrons occupy orbitals in which orbitals are represented
as boxes and electrons are represented as arrows

Question 5

Pauli Exclusion Principle

Answer 5

Each orbital can have a maximum of two electrons, with opposing spins

Question 6

Hund’s Rule

Answer 6

When filling orbitals of equal energy, electrons fill them singly first, with parallel spins

Question 7

Paramagnetic

Answer 7

Atoms or ions with unpaired electrons are paramagnetic, and are attracted to an external
magnetic field

Question 8

Diamagnetic

Answer 8

Atoms with no unpaired electrons are diamagnetic, and are not attracted to an external
magnetic field

Question 9

Valence Electrons and its importance

Answer 9

Electrons in the outermost principal shell of an atom. Valence electrons are held
more loosely, are more easily shared, and play a large role in determining the physical and chemical
properties of an element

Question 10

Core Electrons

Answer 10

Electrons not in the outermost principal shell of an atom

Question 11

Principal Quantum Number (n)

Answer 11

Specifies the principal shell of an orbital. Can be integer values
between 1 and 7

Question 12

Angular Momentum Quantum Number (l)

Answer 12

Determines the shape of an orbital. Can be integer values
between 0 and n-1

Question 13

Magnetic Quantum Number (ml)

Answer 13

Determines the orientation of an orbital. Can be integer values,
including 0, between -l and l

Question 14

Spin Quantum Number (ms)

Answer 14

Specifies the spin of an electron. Two possible spins: up spin (+1⁄2) and
down spin (-½)

Question 15

Effective Nuclear Charge (Zeff)

Answer 15

The net positive charge experienced by an electron in a multi-electron
atom

Question 16

Shielding

Answer 16

Electrons in core orbitals screen valence electrons from the full effect of the nuclear charge

Question 17

Atomic Size and trend

Answer 17

General term to describe the average bonding radius of an atom;
size increase down to the left

Question 18

Ionization Energy and trend

Answer 18

Energy required to remove an electron from an atom or ion in the gaseous state; increase top right

Question 19

First Ionization Energy

Answer 19

Energy required to remove an electron from a neutral atom in the gaseous
state

Question 20

Second Ionization Energy

Answer 20

Energy required to remove a second electron from an already-ionized atom
in the gaseous state

Question 21

metallic character trend

Answer 21

down to left

Question 22

equation for speed of light

Answer 22

c=(wavelength)(Frequency v)

Question 23

Energy of photon equations

Answer 23

E=hv; E=hc/(wavelength)

Question 24

Energy of electron and transition

Answer 24

-2.18 x 10^-18 J (1/n^2)
-2.18 x 10^-18 J [(1/n^2f) - (1/n^2i)]

Question 25

The wavelength of light emitted equation

Answer 25

ΔEatom = -ΔEphoton

Question 26

equation for wavelength for light emitted

Answer 26

wavelength = hc/E

Question 27

Nuclear effective charge equation

Answer 27

Z - S

Question 28

Steps to calculate wavelength of light

Answer 28

find energy of transitions
find energy of photon (multiply by negative
(h)(c)/ energy of photon

Question 29

Isoelectronic ions

Answer 29

The size of isoelectronic ions gets progressively smaller as the atomic number increases
Caused by the larger number of protons