Structure and Properties

Question 1

Aufbau Principle

Answer 1

Orbitals are filled in order of increasing energy

Question 2

Hund’s Rule

Answer 2

Orbitals of a particular sublevel must be half filled with 1e- before the e- are paired

Question 3

Pauli Exclusion Principle

Answer 3

Each orbital can hold a maximum of 2 e- which must be spinning in the opposite direction

Question 4

Orbital Filling Chart

Answer 4

Used to create energy level diagrams

Question 5

How to draw energy level diagrams

Answer 5

Determine the #of e- that need to be placed, follow aufbau principle

Question 6

Energy level diagrams for Anions

Answer 6

ion formed by the addition of e- to the p sublevel until it is full.

Question 7

Energy level diagrams for Cations

Answer 7

A positive ion that is formed by removing e- from s, p, or d sublevels. Removed from the highest principle quantum # and the highest energy level first

Question 8

Electron Configuration

Answer 8

A short hand notation that shows the arrangement of e- in each of the occupied sublevels of an atom or ion. (a simplified way of describing the e-level diagram)

Question 9

Orbital Filling Chart and the Periodic Table

Answer 9

1s, 2s, 2p, 3s, 3p, 4s, 3d 4p, 5s, 4d, 5p, 6s, 5d, 6p, 7s, 6d, La+Ac - 4f + 5f

Question 10

Core Electron Comfigurations

Answer 10

Also known as shorthand e- configurations. Places the noble gas in square brackets at the beginning of the e- configuration (show orbitals when bonding)

Question 11

Anomalous Electron Configurations

Answer 11

For d sublevel only: If possible, e- are promoted from a full s orbital to the d level

Question 12

Lewis Symbols of Atoms

Answer 12

Visual representations of the valence e- in s and p orbitals. ex: O - 2s^2(2p^4), 2+4 = 6e-

Question 13

Atomic Spectra Phenomenon

Answer 13

Sir Issac Newton: lines imply that electronic energy is quantized

Question 14

Bohr and Hydrogen

Answer 14

Succeeded in calculating H+ wavelengths but did not work for larger atoms so original idea of fixed orbit and distance was abandoned

Question 15

Louis de Broglie

Answer 15

1923 - particles are transported by a wave

Question 16

Werner Heisenburg

Answer 16

1927 - you cannot know the position and velocity of a particle

Question 17

Erwin Schrodinger

Answer 17

1926 - developed equations that describe motion of an e-

Question 18

1st Quantum #: Principle Quantum # (n)

Answer 18

e- are located in energy levels or shells and are identified by a PQ#. n can be any value from 1 to infinity and describes the orbital size and energy. the greater the n, the further an e- from the nucleus

Question 19

2nd Quantum #: Sublevels (l)

Answer 19

each n contains sublevels of slightly differing energies, identified by a letter -s, p, d or f. (s-sharp, p-principle, d-diffuse, f-fundamental). L = 0-(n-1)

Question 20

3rd Quantum #: Orbitals [m(l)]

Answer 20

each sublevel contains a certain # of orbitals, each holding max of 2e-.

Question 21

4th Q#: Spin

Answer 21

each e- has opposite spins in one orbital

Question 22

What is an Orbital

Answer 22

A 3D region of space aound the nucleus of an atom where the probability of finding an e- is high.

Question 23

Magnetic Quantum # m (l)

Answer 23

Each sublevel contains a certain # of orbitals with a specific orientation m (l)= -l -> +l

Question 24

Types of Bonds

Answer 24

Ionic: EN=1.7-3.3
Covalent: EN=0-0.2
Non-polar: EN=0.3-1.6
Metallic: sea of electrons

Question 25

VSEPR

2-1, 3-1, 2-2, 4-1, 3-2, 5-1, 4-2, 3-3

Answer 25

2-1: Bent. 3-1: trigonal pyramidal. 2-2: Bent. 4-1: seesaw. 3-2: Tshaped. 5-1: square-based pyramidal. 4-2: square planar. 3-3: Tshaped.

Question 26

Valence Bond Theory

Answer 26

Orbits overlap to form new orbital w/ opposite spin e-.

Question 27

Sigma Bond

Answer 27

Direct end to end overlap of s or p orbitals. Single covalent bond is always sigma bond.

Question 28

Pi Bond

Answer 28

Two parallel orbitals share a pair of e-. (Double covalent is shorter and stronger than single covalent)

Question 29

How many sigma and pi?
Single bond
Double bond
Triple bond

Answer 29

Single: 1sigma
Double: 1sigma,1pi
Triple: 1sigma,2pi

Question 30

Polar covalent bonds

Answer 30

E- pair is shared unequally, most closer to atom w/ higher EN, formation of dipoles

Question 31

Free Radicals (Paramagnetic)

Answer 31

contain a single unpaired e- in the structure

Question 32

Resonance Structures

Answer 32

Two or more Lewis structures that show the same relative position of atoms but different position of double/triple bonds

Question 33

Coordinate covalent bonds

Answer 33

a bond in which the shared pair of e- is contributed by one atom and an atom/ion that requires 2e- to complete it’s s or p sublevel

Question 34

Hybrid Orbitals

Answer 34

when an e- from a full orbital is promoted to an empty orbital of higher energy in same PQ# occurs in the bonding process