Where did the elements come from?

Where did the elements come from?

Hydrogen, a little helium and an even

smaller amount of lithium were created in

the big bang. The universe is about 95%

hydrogen. Clouds of hydrogen gas and dust

are compressed by gravity into stars. When

a star's core runs out of hydrogen, the

nuclear reaction pauses, and gravity

Where did the elements come from?

◻

If the star is big enough it can eventually

create all the elements in the periodic

table up to iron (through nuclear

reactions and gravity). If a giant star

explodes (supernova), it will release

The most common Elements in the

Earth’s CRUST

Element

Amount

Oxygen 46.1 %

Silicon 28.2 %

Aluminum 8.23 %

Iron 5.63 %

The most common Elements in the

Earth’s OCEANS

Element

Amount

Oxygen 85.84 %

Hydrogen 10.82 %

Chlorine 1.94 %

Sodium 1.08 %

The most common Elements in the

Earth’s ATMOSPHERE

Element

Amount

Nitrogen 78.1 %

Oxygen 20.9 %

ATOMS !!!

What are the 3 subatomic particles?

Protons

Neutrons

Electrons

What are the charges of the subatomic

particles?

protons (+)

neutrons

(0)

electrons

(-)

We know that there are the same number of p+ and e- in atoms on the Periodic Table… So What is the

overall charge of any atom?

The overall charge of any atom is

NEUTRAL… the positive

charge cancels out the

What are the masses (amu) of the subatomic

particles?

p

= 1amu

n = 1amu

e

= 0 amu

_{1.66 x 10}

_{kg = 1 amu}

What is this AMU

stuff?????

Atomic mass unit

(AMU)

What are the two areas of an atom?

Nucleus

P+ & No

Where are the p+, n, and e- located in an

atom?

p+

in the nucleus

n

o

in the nucleus

e-

in the electron cloud

Nucleus

Where is ALL the mass in an atom

located?

Where is most of the volume of an atom

located?

The nucleus contains the p+ and n… while the electrons “orbit” the nucleus in the energy rings of the e- cloud.

So what are the charges of the

different areas?

1. So what is the overall charge of the nucleus?

Positive

2. So what is the overall charge of the electron cloud?

Negative

QUICK REVIEW- ATOMS

Sub-atomic particles:.

particles charge amu location abbrev.

Protons

Electrons

e-Neutral (0)

+ nucleus p+

0 1 1 neutrons Electron cloud _

nucleus no

protons, neutrons, and electrons nucleus and electron cloud

Energy Levels of the Atom

8

2e- 8 e- 32e- 18 18 32e-The Nucleus

P+ N0

1st shell 7th shell 2nd shell 3rd shell 4th shell 5th shell 6th shell

Beginning with Bohr Models

◻ Let’s try a few easy bohr models:

Li

Bohr Model Practice

1. Ca

2. O

3. Ne

4. K

5.

Rb

More Bohr Model Practice

11. Fr

12. Te

13. Sn

14. Cs

15. Kr

Complete the Bohr Models for the following

elements.

Ne

,

Ar,

Kr

and

Xe

◻ What 4 patterns or

trends did you notice they have in common?

◻ “Predict” what you think Radon’s (Rn) bohr model would look like.

◻ Six rings ◻ Full shell

◻ More massive

◻ All of the rings or

shells are full.

◻ They are all in the

same group (18)

◻ They gain an energy ring as you go down a period.

◻ They gain more

Lets take a look at the Periodic

Table!

Patterns from the Bohr Models

Even More Bohr Model Practice!

21. Os

22. Hf

23. Cm

24. Sr

25. Ho

26. Tc

27. Ac

28. Zr

29. Po

30. Np

Bohr Model

H

vs.

He

Explain why we use helium filled balloons

instead hydrogen filled balloons at Parties.

Hydrogen is unstable and

flammable and helium is stable!

Energy rings are not filled

Energy rings are filled

“

Life on the Edge”

with

Valence Electrons

Valence electrons are electrons in the outermost shell of an atom.

They determine whether the atom will bond with another atom.

How many valence electrons does

lithium have here?

1 valence electron

Arrangement of the Periodic

Table

1. What atom is this?

Oxygen

2. Which subatomic “particle” helped you to

determine that this Bohr model was of oxygen?

Arrangement of the Periodic

Table

1. The periodic table is arranged according to what? A. Atomic Symbol

B. Atomic mass C. Atomic number

D. Number of Energy Shells

◻ Do the elements on the periodic table all increase

according to their masses?

Periodic Table Card Sort Poster

Breaking the Code

Purpose

of the patterns that are contained in the periodic table of elements.

Do you notice any patterns here as you move

down a column on the Periodic Table?

Li

_Na

_K

_Rb

Can you “predict” how many energy rings a bohr model of Francium (Fr) would have?

Gaining more mass

Gaining more energy rings Gaining more

Francium (Fr) Bohr Model

Seven energy rings

1

What Bohr model patterns are you

starting to see develop?

◻ Periodic Table Patterns

◻ The atomic number is the same number as the

number of protons and electrons.

◻ Atoms get larger as you move down and to the right on the periodic table.

◻ As you move from left to right on the periodic

table, you gain protons and electrons and neutrons.

◻ As you go down from the periodic table, the atom

Metals vs. Non-Metals

Metals

Non-metals

Man made elements and Rare Earth metals

Metalloids on the Periodic

Table

FAMILIES/ GROUPS

Periods/ Rows

Properties of Metals

◻ Most elements are metals. 88 elements to the left of the stairstep line are metals or metal-like elements.

◻ Tend to have Luster

◻ High density ◻ Ductile

◻ Malleable

(shininess) (heavy for their

size)

Properties of Non-metals

◻ Nonmetals are found to the right of the stair step line.

◻ No luster ◻ Brittle

◻ Not ductile

◻ Not malleable

(dull)

Properties of Metalloids

◻ Metalloids are elements on both sides of the stair step line. They have properties of both metals and nonmetals.

◻ Solids

◻ Can be shiny or dull ◻ Ductile

So where do the names come

from?

Iron

(Fe)………….……Ferrum

Sodium (Na)….. …….Natrium

Gold (Au)………Aurum Silver (Ag)………….Argentum Potassium (K)………… Kalium Copper (Cu) ………….Cuprum Mercury (Hg) ……Hydragyrum Antimony (Sb)………… Stibium Tin(Sn)….………… Stannum Lead(Pb) ………..Plumbum Tungsten(W)………….Wolfran

Steps for creating a Bohr model

1. Complete the particle

inventory for the atom (protons, electrons and neutrons).

2. Draw your nucleus.

3. Put the number of protons and neutrons in the nucleus.

4. Circle how many electrons you need to use in the shells.

5. Know how many electrons and shells you will need.

6. Put 2 electrons in the first

shell. If there are more than 2, begin to fill the next shell

(maximum of 8).

7. You cannot begin to fill the next shell until the previous shell is filled.

8. Remember` how many

electrons each shell can hold a maximum of.

Element Atomic Number Atomic Mass # of Protons # of Electrons # of Neutrons

Zn

Xe

Au

Hg

I

Manganese

First Energy Level: 2

Second Energy

Level: 8

Third Energy Level:

8

Fourth Energy

Level: 7

Yttrium

First Energy Level: 2

Second Energy

Level: 8

Third Energy Level:

8

Fourth Energy

Level: 18

Fifth Energy Level:

3 P39 N50

2e 8e 8e 18e 3e

P25 N30

2e 8e 8e 7e

Krypton

First Energy Level: 2

Second Energy

Level: 8

Third Energy Level:

8

Fourth Energy

Level: 18

Germanium

First Energy Level: 2

Second Energy

Level: 8

Third Energy Level:

8

Fourth Energy

Level: 14

Krypton Germanium

P36 N48

2e 8e 8e 18e

P39 N50