KWL CHART--ELECTRONS WHAT DO I ALREADY KNOW ABOUT ELECTRONS?

WHAT DO I WANT TO KNOW CONCERNING ELECTRONS?

WHAT HAVE I LEARNED TODAY ABOUT ELECTRONS?

GPS STANDARD SC3. Students will use the modern atomic theory to

explain the characteristics of atoms.

b. Use the orbital configuration of neutral atoms to explain its effect on the atom’s chemical properties.

f. Relate light emission and the movement of electrons to element identification

ELECTROMAGNETIC SPECTRUM In order of increasing energy:

Radio, microwaves, infrared, visible light, uv, xrays, gamma, cosmic

Facts About Electrons 1.They can only move certain distances from the nucleus.

2.They can only move at certain speeds.

3. They give off (release) energy when moving to a lower level and gain energy (absorb) when moving to a higher level.

4.They cannot jump down to a level with a full octet of electrons.

The Bohr Model He said that electrons occupy definite energy levels

around the nucleus.

However, exact locations of electrons are not known because they are constantly moving due to the loss/gain of energy.

Therefore, these locations are only highly likely places to find electrons at a certain time.

Photons They are bundles or packets of energy

When an atom gains photons, it becomes excited and the electrons move to a higher energy level.

When it loses photons, it gives off energy, and electrons move to lower level (ground state).

Atoms become excited ( and gain photons) by heating them or passing electricity through them. When they lose these photons, the electrons give off color, depending on amount of energy given off (related to frequency and wavelength).

Wave Characteristics WAVELENGTH—distance from crest to crest or trough

to trough

FREQUENCY—# of waves passing a certain point per second ; is measured in Hertz (Hz)

AMPLITUDE—the height or depth of a wave

SPEED—is determined by wavelength & freq.

All electromagnetic waves travel at the speed of light (300,000,000 m/sec)

Valence electrons Involved in chemical bonding & chemical reactions

For an A group element, this is equal to the A group #

Lewis Dot Diagrams Show the outermost(valence) electrons for an atom

Ex: Li N

Be O

B F

C Ne (has an OCTET)

You try…… As He

Kr Al

Sr Br

Ra Cs

Pb

TICKET OUT Draw the electron dot symbols for:

1. Na

2. P

3. Ar

4. S

5. Mg

6. He

Activity—Periodic Pyramid Color each row of your periodic pyramid the color listed below. Make sure to color starting at the Beginning of that row THROUGHOUT the End of that row. Row 1 = red (H all the way to the end) Row 2 = orange (Li through Ne) Row 3 = yellow (Na through Ar) Row 4 = green (K through Kr) Row 5 = blue (Rb through Xe) Row 6 = dark purple (Cs through Rn) Row 7 = light purple (Fr through #118) ***choose 4 DISTINCTLY different colors to color the “s” “f”, “d”, and “p” labels at the top of the pyramid

***cut off all the black portion. Do not detach the base of the pyramid. Tape the sections together that say “glue/tape”. Create your pyramid!!

Electron Energy Levels & Sublevels Electrons are located within the atom outside the

nucleus on energy levels. Within these energy levels are sublevels.

Possible sublevels in order of increasing energy: s,p,d,f

Elements are located within the s, p, d, and f blocks on the periodic table (this represents which sublevel these elements’ valence electrons are on)

These sublevels are used to write an atom’s electron configuration

Electron Configurations—Rows 1-3 Show the electron arrangement within the electron cloud

on certain energy levels and sublevels Ex: Hydrogen--1s1

Helium--1s2 Lithium—1s2 2s1

Beryllium– 1s2 2s2

Boron – 1s2 2s2 2p1

Oxygen --1s2 2s2 2p4

Neon—1s2 2s2 2p6

You try……. (configurations & dots) Nitrogen Fluorine

Sodium

Phosphorus

You try….. (configurations & dots)

Argon

Sulfur

Aluminum

magnesium

In Educreations APP…. Write the electron configuration AND draw the

electron dot for:

Cl

Ca

N

Si

Electron Configurations (Rows 4-5) On these 2 rows, you encounter the d sublevel

The d sublevel is always minus 1 from the row it’s on

For example, row 4 contains 3d and row 5 contains 4d

The Lewis dot symbol will only contain the valence s and p electrons

Ex:

Calcium (Ca) 1s2 2s2 2p6 3s2 3p6 4s2

Iron (Fe) 1s2 2s2 2p6 3s2 3p6 4s2 3d6

Copper (Cu) 1s2 2s2 2p6 3s2 3p6 4s2 3d9

Bromine (Br) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

You try (configurations & dots)…… Rubidium (Rb)

Silver (Ag)

Tin (Sn)

Antimony (Sb)

Electron Configurations (Rows 6 & 7) On these rows you first encounter the f sublevel.

The f sublevel is always minus 2 from the row it’s on.

For example: row 6 contains 4f, and row 7 contains 5f

The Lewis dot symbol will only contain the valence s and p electrons

Ex:

Europium (Eu) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f7

Tungsten (W)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d4

Radon (Rn) 1s2 2s2 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6

Californium (Cf) 1s2 2s2 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f 10

You try….. (configurations & dots)

Mercury (Hg)

Curium (Cm)

Rutherfordium (Rf)

Abbreviated Configurations Uses the previous noble gas written in brackets

and the configuration that is only part of the row it is on

This eliminates you from having to start all the way back at 1s

Ex:

Ca (Ar) 4s2

Ag ( Kr) 5s2 4d10