2-Electron Configuration.pptx

(1)

Objectives

You will be able to write the atomic symbol for all elements of the periodic table.

You will be able to determine the amount of protons, neutrons, and electrons in an

element.

1/6/21 1

(2)

Atomic Number

Atoms are composed of identical protons, neutrons, and electrons



_{How then are atoms of one}

element different from another

element?

Elements are different because they contain different numbers of PROTONS

The “atomic number” of an element is the number of protons in the nucleus

(3)

Atomic Number

Atomic number (Z) of an element is

the number of protons in the nucleus

of each atom of that element.

Element

# of protons Atomic # (Z)

Carbon

6

6 Phosphorus

15

(4)

Mass Number

Mass number is the number of

protons

and

neutrons

in the nucleus of an

isotope:

Mass # = p

+

+ n

0

Nuclide

p

+

n

0

e

-

Mass #

Oxygen

₈

33 42

31

15

8 8 16

16

Arsenic

75 33 ₇₅

(5)

Complete Symbols

Contain the symbol of the

element, the mass number and

the atomic number.

X

Mass

number

Atomic

number

Subscript →

(6)

Symbols

We can also put the mass number

after

the name of the element:



_carbon-12

(7)

Symbols

Find each of these:

a) number of protons

b) number of

neutrons

c) number of

electrons

d) Atomic number

e) Mass Number

Br

80

35

(8)

Symbols

Find each of these:

a) number of protons

b) number of

neutrons

c) number of

electrons

d) Atomic number

e) Mass Number

Hg

200

80

(9)

Symbols



If an element has an atomic

number of

34 and a mass

number of

78 , what is the:

a) number of protons

b) number of neutrons

c) number of electrons

d) complete symbol

(10)

Tell your neighbor

How can you determine the amount of neutrons an element has?

How can you determine the number of protons an element has?

How can you determine the number of electrons an element has?

(11)

Warm up: Fill me Out

Nuclide p

+

n

0

e

-

Atomic Symbol

Vanadium

Actinium 49

51

154

Ho

(12)

(13)

Objectives

_{You will be able to write the orbital}

configuration, and electron configuration of a given element.

_{Given an electron configuration, you will be}

able to determine which element on the

periodic table corresponds to the configuration.

_{You will be able to define what a valence}

electron is.

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(14)

Electron Configuration

“The Blocks”

s

p

d

(15)

s-block

1st Period

1s

1 1st column

of s-block

Lets look at a configuration

Example -

Hydrogen

1 2 3 4 5 6 7

(16)

1s

2 2s

2 2p

3 And another example…

Example -

Nitrogen

1

2 3 4 5 6 7

(17)

Periodic Patterns

Period #

energy level (subtract for d & f)

A Group #

total # of valence e

-Column within sublevel block

(18)

Electron

Configuration

(19)

What the sublevels/orbitals look like

1

3

5

(20)

The Sublevel's

The “

s

” block has one (1) orbital

The “

p

” block has three (3) orbital's

The “

d

” block has five (5) orbital's

The “

f

” block has seven (7) orbital's

(21)

General Rules

Pauli Exclusion Principle

No two electrons in the same atom can

have the same set of 4 quantum

numbers.

That is, each electron in an atom has a

unique address of quantum numbers.

(22)

General Rules

Pauli Exclusion Principle

Each orbital can hold TWO (2)

electrons with

opposite

spins.

(23)

General Rules: Filling Order

Aufbau

Principle

e

-

fill the

lowest energy

orbitals first.

(24)

RIGHT

WRONG

General Rules

Hund’s Rule

Within a sublevel, place one e

-

per

orbital before pairing them.

(25)

O

8e

-Orbital Configuration: Uses arrows

Electron Configuration:

Uses super scripts

1s

2 2s

2 2p

4 Notation

(26)

C

6e

-Orbital Configuration: Uses arrows

Electron Configuration:

Uses super scripts

1s

2 2s

2 2p

2 Notation

(27)

Lets Practice Orbital Notation

On your worksheets provided, draw the orbital notation for the following:

_Fluorine Calcium Silicon Silver Iodine _Copper Sulfur

(28)

Shorthand Configuration

S 16e

-Valence Electrons

Core Electrons

S16e

-

[Ne]

3s

2

3p

4

1s

2

2s

2

2p

6

3s

2

3p

4

Notation

(29)

Valence electrons

are the

electrons

contained in the outermost, or

“

valence”

,

electron

shell of an atom.

They are involved in the bonding

between atoms

(30)

s

_{d (n-1)}

f (n-2)

p

Periodic Patterns

Shorthand Configuration

Core e

-

:

Go up one row and over to the

Noble Gas.

Valence e

-

:

On the next row, fill in the #

of e

-

in each sublevel.

1 2 3 4 5 6 7

(31)

[Ar]

4s

2 3d

10 4p

2 Periodic Patterns

Example -

Germanium

1 2 3 4 5 6 7

(32)

s

_p

d (n-1)

f (n-2)

1 2 3 4 5 6 7 6 7 Periodic Patterns

(33)

Give the Shorthand Configuration for

P

Br

1s

2

2s

2

2p

6

3s

2

3p

3

Practice…

Give the Longhand Configuration for

15e

(34)

Practice

What is the short hand electron

configuration for the following

elements, and list the number

of valence e

-

for each;

(35)

Single

Atom

Lewis Structures

What do they look like?

Procedure

1. Write element symbol

2. Add valence electrons (dots) around

element symbol

How can we determine valence

electron with out writing the electron

configuration

If valence electrons are paired in an

orbital, pair them on the structure, if

not, do not pair (keep them single)

(36)

Valence Electrons

How many valence

electrons do the following

atoms have?

(37)

Single

Atom

Lewis Structures

Procedure

1. Write element symbol: O

2. Add valence electrons (dots) around

element symbol.

Oxygen has 6

valence electrons

O

S

P

(38)

Single

Atom

Lewis Structures

Lets try another:

As

Identify the number of valance electrons ____

(39)