NOTES Out 1-3 Dots, Met-nonmet, Oxidation.doc

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I. Outcome 1 – Lewis Dot Structures (electron dot

diagrams)

Lewis Dot Structures / Electron Dot Diagrams – Used to show the number of valence electrons for an atom of an element.

>> Dots are used to represent each valence electron.

Example1: Na has ____ valence electrons

Electron dot diagram for Na

Na

Example 2: Sulfur (S) has ____ valence electrons

Electron dot diagram for S

S

Example 3: Neon (Ne) has ____ valence electrons

Electron dot diagram for Ne

Ne

Octet Rule

: Atoms tend to gain, lose or share electrons to get eight electrons in the last energy level.

The Lewis dot diagrams and the chemical bonding of

Sodium (Na) and Chlorine (Cl)

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II. Outcome 2 & 3 – Families of Elements & Oxidation

Numbers.

A) Columns (vertical) on the PTE are called FAMILIES or GROUPS.

1) Families on the PTE are numbered: 1, 2, 3-12, 13, 14, 15, 16, 17, 18)

2) Elements in a family (same column) have similar properties.

B) Rows (horizontal) on the PTE are called PERIODS. 1) On the PTE there are 7 periods.

2) Elements in a period do NOT have similar properties.

++ Atoms are “happy” when they have full

energy levels.

++ So, their goal is to create full energy levels.

C) NONMETALS – Elements to the right of the stair-step line on the PTE.

1) Nonmetals are “electron takers.” Meaning, they take electrons from other atoms to fill their energy levels. 2) Taking electrons creates a negative (-) ion.

Ion = charged atom.

Oxidation Number – Charge of the ion.

Ex: Chlorine (Cl) has 7 valence electrons. It takes 1 electron to fill its outer energy level. So, Cl has a -1 charge. Written as an oxidation number: Cl

-D) METALS - Elements to the left of the stair-step line on the PTE.

1) Metals are “electron givers.” Meaning, they give away electrons to other atoms to get to full energy levels. 2) Giving electrons creates a positive (-) ion.

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E) METALLOIDS – Elements that are in full contact with the stair-step line on the PTE. EXCEPTION: Aluminum is a metal.

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I. Outcome 1 – Lewis Dot Structures (electron dot

diagrams)

Lewis Dot Structures / Electron Dot Diagrams –

Used to show the number of

valence electrons

for an atom of an element.

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Lewis Dot Structures / Electron Dot Diagrams – Used to show the number of valence electrons for an atom of an element.

>> Dots are used to represent each valence electron.

Example1: Na has ____ valence electrons

Electron dot diagram for Na

Na

Example 2: Sulfur (S) has ____ valence electrons

Electron dot diagram for S

S

Example 3: Neon (Ne) has ____ valence electrons

Electron dot diagram for Ne

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Octet Rule

:

Atoms tend to gain, lose or share

electrons to get

eight

electrons in the last energy

level

.

The Lewis dot diagrams and the chemical bonding of

Sodium (Na) and Chlorine (Cl)

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1) Families on the PTE are

numbered:

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1) Families on the PTE are numbered: 1, 2, 3-12, 13, 14, 15, 16, 17, 18

2) Elements in a family (same

column) have similar

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B) Rows (horizontal) on the PTE are called PERIODS.

1) On the PTE there are 7

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B) Rows (horizontal) on the PTE are called PERIODS.

1) On the PTE there are 7 periods.

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B) Rows (horizontal) on the PTE are called PERIODS. 1) On the PTE there are 7 periods.

2) Elements in a period do NOT have similar properties.

++ Atoms are

“

happy

”, “

content

”,

“

satisfied

”

when they have full

energy levels and are

electrically neutral (

no charge

).

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C) NONMETALS – Elements to

the right of the stair-step

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1) Nonmetals are “electron

takers.”

Meaning, they take

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1) Nonmetals are “electron takers.” Meaning, they take electrons from other atoms to fill their energy levels.

2) Taking electrons creates a

negative (-) ion.

Ion = charged atom.

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1) Nonmetals are “electron takers.” Meaning, they take electrons from other atoms to fill their energy levels. 2) Taking electrons creates a negative (-) ion.

Ion = charged atom.

Oxidation Number – Charge of the

ion.

Example 1

:

Chlorine (Cl) has 7 valence

electrons.

It takes

____electron

to fill its

outer energy level.

So, Cl has a ____ charge.

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Ex 1: Chlorine (Cl) has 7 valence electrons. It takes 1 electron to fill its outer energy level. So, Cl has a -1 charge. oxidation number : Cl

-Example 2:

Oxygen =

_____

valence, takes

____

electrons, has a

____

charge and an

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D) METALS - Elements to the left of the stair-step line on the PTE.

1) Metals are “

electron givers

.”

Meaning, they

give away

ALL

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1) Metals are “electron givers.” Meaning, they give away all valence electrons to other atoms to get to full energy levels.

2) Giving away electrons

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1) Metals are “electron givers.” Meaning, they give away electrons to other atoms to get to full energy levels. 2) Giving electrons creates a positive (+) ion.

Ex 1: Na has

1 valence electron

.

It easily gives

____electron

away.

So, Na has a charge of

______

.

Written as an oxidation

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2) Giving electrons creates a positive (-) ion.

Ex1: Na has 1 valence electron. It easily gives 1

electron away. So, Na has a charge of +1. oxidation number: Na+

Example 2: Ca =

_____

valence

electron,

gives away

_____

electrons,

has a

_____

charge,

and an oxidation number of

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Example 2: Ca = 2 valence electron, gives away 2 electrons,

has a +2 charge, and an oxidation number of Ca+2

E)

METALLOIDS

– Elements that are

in

full contact

with the

stair-step

line

on the PTE.

+ Have properties of

metals

and

nonmetals

.

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F)

FAMILIES OF METALS, NONMETALS &

METALLOIDS:

METALS

(3 FAMILIES)

# of valence

Family

Name of Family

Family #

electrons

members

Alkali Metals

Alkaline Earth Metals

Transition Metals

List as many PROPERTIES of metals as you can find:

METALLOIDS

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NONMETALS

(6 FAMILIES)

# of valence

Family

Name of Family

Family #

electrons

members

Boron Family Carbon Family Nitrogen Family Oxygen Family Halogens Nobel Gases