Chemistry - Chapter 5 and 6

Wavelength

Wavelength

The distance between two waves

Amplitude

The height of a wave

Frequency

How often a wave goes up and down

The speed of light

c = 3.0 x 10^8 m/s

FOR THE LEFT SIDE: say if it has (short or long) or (lowest or highest): wavelength, energy, and frequency

Short Wavelength High energy High frequency

FOR THE RIGHT SIDE: say if it has (short or long) or (lowest or highest): wavelength, energy, and frequency

Long Wavelength Low energy Low frequency

FOR THE LEFT SIDE: say if it has (short or long) or (least or most) (lowest or highest): wavelength, energy, and frequency

Short wavelength Most energy Highest frequency

FOR THE RIGHT SIDE: say if it has (short or long) or (least or most) (lowest or highest): wavelength, energy, and frequency

Long wavelength Least energy Lowest frequency

In order for an electron to move to another level they have to...

...absorb a specific amount of energy

Excited State

When electrons absorbs energy and moves to a higher energy level

Ground State

When electrons "fall" back to their original energy level, they release light

Are excited states stable or unstable?

Unstable

How does the Emission Spectra connect to changing the color of light?

The higher the fall the more energy is released, changing the color of light produced.

What are the 3 rules for Electron Configurations?

• Aufbau principle • Pauli Exclusion Principle • Hund’s Rule

Aufbau

Electrons occupy orbitals of lower energy first.

Pauli Exclusion Principle

An orbital can hold only two electrons and they must have opposite spin.

Hund's Rule

In a set of orbitals, the electrons will fill the orbitals in a way that would give the maximum number of parallel spins (maximum number of unpaired electrons).

In the configuration: 1s^2, what does 1 mean?

The MAIN energy level

In the configuration: 1s^2, what does "s" mean?

Sublevels

In the configuration: 1s^2, what does ^2 mean?

Number of electrons in the sublevel

What is the block for the blue area?

s

What is the block for the red area?

d

What is the block for the orange area?

p

What is the block for the green area?

f

How to calculate the noble gas abbreviation.

1. Use the last noble gas that is located in the periodic table right before the element.

2. Write the symbol of the noble gas in brackets.

3. Write the remaining configuration after the brackets. Ex: Fluorine: [He] 2s^2 2p^5

A family is a ? on the periodic table

Column

Where are the alkali metals?

First column

Where are the alkaline earth metals?

Second column

Where are the transition metals?

Middle section

Where are the metalloids?

Staircase

Where are the halogens?

Second to last column

Where are the noble gases?

Last column

Atomic radius

the size of the atom. PLURAL : Atomic radii

Atomic radius gets (smaller/larger) going down a group and why?

Larger, because we are adding another valence shell.

Atom raduis get (smaller/larger) across a period and why?

Smaller, because the charge in the nucleus is increasing.

Electronegativity

A measure of the attraction an atom has for electrons when bonded.

Electronegativity gets (smaller/larger) going down a group.

Smaller

Electronegativity gets (smaller/larger) going across.

Larger

Which element has the most electronegativity?

F (Fluorine) has the greatest electronegativity at 4.0

Ionization Energy

The energy required to remove an electron from a gaseous atom or ion.

Ionization Energy gets (smaller/larger) going across.

Larger

Ionization Energy gets (smaller/larger) going down.

Smaller

Electron Affinity

Energy released when an electron is added to the atom.

Electron shielding

Atoms with more energy levels can't hold onto their valence electrons as strongly. The pull from the nucleus is partially blocked by each layer of electrons.

(Easier/harder) to remove an electron with more shielding?

Easier

Cation

When atoms lose valence electrons, they become positively charged ions.

Cations are always (smaller/larger) than the original atom.

Smaller

Anions

Atoms that gain electrons become negatively charged ions. Atoms gain electrons in their outermost shell.

Anions are always (smaller/larger) than the original atom.

Larger

Most reactive NON-metal?

Fluorine - F

Most reactive METAL?

Francium - Fr