Atomic Structure Revision

SAMPLE ONLY SAMPLE ONLY SAMPLE ONLY

For FULL presentation click HERE >> www.warnescience.net

Atomic Structure

K Warne

http://www.warnescience.net/




Elements

ELEMENTS - cannot be broken up into simpler

substances.

- their smallest particles are atoms.

- they are found on the periodic table.

elementatom





Chlorine:

• _________

• _________

• _______

Compounds

Sodium:

• ______

• _______

• Very _______

ClNa

Elements

Compound (can be chemically

broken down into two original elements)

NaCl molecule

Different to original atoms

REACTION

• Energy ________

• Atoms ________

NaCl

Sodium Chloride

• ______________

• ______________.

• ______________





The AtomAn atom consists

of a NUCLEUS made of ……………..and ………………

………………….orbit the nucleus at high speed.

Helium atom

The electrons are ……………… charged - the

protons are ………………….

The number of electrons is always …………

to the number of protons.

e-

Proton (….)

Electron (....)e-

Neutron (….)

++

The element is determined by the number of ………………!!

charge





THE NEUTRAL ATOM• Atomic Number (_) = number of ______

• Mass number (…) = ________ + ________.

• Number of neutrons = ______

Notation

Z

A

X………. Number

(_________)

………… Number

(________) symbol

e-

proton

electrone-

neutron





Atomic Structure

Symbol

NotationName Protons Neutrons

Mass

NumberElectrons

4020Ca Calcium 20

40-20 =

2040 20

3115P

14 28

12 6

Mg





Isotopes

…………………

Atoms of the ……. ………….. which have …………. ………… of ………………. Others – Boron …….., Hydrogen …..….., Chlorine ……………………... Write notation and work out numbers of neutrons in each of these.

+

+

+

++

e- e-

e- e-e-

e-

++

+

+

++

e- e-

e- e-e-

e-

The two carbon atoms below both are not identical – can you spot what

is different? (Write down A and Z in the symbol notations.)

……..C …

…..C

+





IsotopesBoron 10 & 11, Hydrogen 1 & 2, Chlorine 35 & 37

510B 5

11B5 neutrons! 6 neutrons!

11H 1

2H0 neutrons! 1 neutrons!

1735Cl 17

37Cl18 neutrons! 20 neutrons!





ISOTOPES

Symbol PROTONS ELECTRONS NEUTRONS

Carbon 1212

6C 6 6 6

Carbon 1313

6C 6 6 7

Boron 1010

5B 5 5 5

Boron 1111

5B 5 5 6

Hydrogen 1

Hydrogen 2

Chlorine 35

Chlorine 37





• Electrons orbit the nucleus in various __________________.

• These levels ______________ from the nucleus.

• Levels further from the nucleus have _____________ _______.

• The OUTERMOST LEVEL is called the _______________ energy level.

• The electrons in the OUTER ENERGY LEVEL are known as the _________________ ELECTRONS.

• The number of valence electronsfor any element is equal to it’s _______________ NUMBER on the periodic table.

e-

e-

e-e-

This atom has _____

valence electrons.

The number of valence electrons of the

following elements are:

• Oxygen:

• Hydrogen:

• Sodium:

• Chlorine:

• Carbon:

Energy levels





Full Shells- Maximum Electrons

• The FIRST or innermost shell as having a maximum of 2 electrons.

• The next two shells have a maximum of 8 electrons each.

• The FOURTH shell can take many more electrons but we shall only consider elements up to the first TWENTY.

2

1

8

7

3

4

5

6

1 2

At Junior Level we can take:

2 + 8 + 8 + (2) = 20

Atomic No = total electrons

Group number = valence

electrons (outer shell)

Valency = no

electrons lost or

gained to get a full

outer shell

K L M N





2s

1s

8 p

8 n

Oxygen

8

O

16

Valence Electrons

Valence electrons are those which are found in the outer

energy level or shell.

An oxygen atom has 8 electrons in total – 6 of which would be in its

outer energy level. The number of valenc electrons in an atom of

oxygen is therefore 6.

O 1s2 2s2 2p4

2p

1

2

3

4

5

6





VALENCY – BOHR DIAGRAMS

Valency – ……………….. of electrons ……..….. or ………....

to have a FULL valence level. (Outer shell)

H He

Li Be B C N O F Ne

Valence electrons – those in ……………. shell.

Na Mg Al Si P S Cl Ar

Mass INCREASES from Left to Right! More

Protons and more electrons!

1 2 ....





15p

16 N

Phosphorus

15

P

31

Bohr Diagram for Phosphorus





VALENCY

• Valency – number of electrons lost or gained to have a FULL valence level. (Outer shell)

Valence electrons – those in outer shell.

Group No I II III IV V VI VII VIII

Valence

electrons

Valency





Valency

• The …………. of an element is the number of ………….. it must ……….. gain or lose to get a full outer shell (8 electrons).

• For METALS the valency is just equal to the ………… ………………..

• For NON-Metals the valency is equal to ……………………….

This atom has a

valency of -2.

The valencies of the following

elements are:

• Oxygen:

• Hydrogen:

• Sodium:

• Chlorine:

• Carbon:





Name Symbol Z A N e- G.No Valence e- Valency

sodium Na 11 23 12 11 I 1 1

Mg

Al

Si

phosphor

us31

15P 15 31 16 15 V 5 -3

32___ 16 32

35___ 17

18

----- Ca





Periodic Table Investigation• On the supplied blank outline of the periodic table.

• Type in symbols for all the elements you know of which are:

– Metals

– Gasses

– Liquids

– Non Metals (substances that are not metals)

Use some form of colour scheme to distinguish the various kinds of elements.

Interactive Periodic Tables you may wish to use:

www.ptable.com

http://www.webelements.com/

Identify any possible trends in the layout of elements.



http://www.ptable.com/

http://www.webelements.com/



The Periodic TableInteractive Periodic Table; www.ptable.comI II <--GROUP NUMBERS--> III IV V VI VII 0

1 2

H He

1 KEY 4

3 4 Atomic number 3 5 6 7 8 9 10

Li BeLi Symbol B C N O F Ne

7 9 Mass number 7 11 12 14 16 19 20

11 12 13 14 15 16 17 18

Na Mg Al Si P S Cl Ar

23 24 27 28 31 32 35.5 40

19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36

K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr

39 40 45 48 51 52 55 56 59 59 64 65 70 73 75 79 80 84

37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54

Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe

86 88 89 91 93 96 99 101 103 106 108 112 115 119 122 128 127 131

55 56 57 * 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86

Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn

133 137 139 179 181 184 186 190 192 195 197 201 204 207 209 210 210 222

87 88 89

Fr Ra Ac

223 226 227

* 58 - 71 Lanthanides58 59 60 61 62 63 64 65 66 67 68 69 70 71

Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu

140 141 144 145 150 152 157 159 163 165 167 169 173 175

90 - 103 Actinides90 91 92 93 94 95 96 97 98 99 100 101 102 103

Th Pa U Np Pu AmCm Bk Cf Es Fm Nd No Lr

232 231 238 237 239 243 247 247 252 (252) (257) (258) (259) (260)





The Periodic TableInteractive Periodic Table; www.ptable.comGI Metals – light grey, react vigorously with water –

release Hydrogen gas – reaction gets more vigorous

as you go down the group.

GVII HALOGENS toxic reactive gases, liquids & solids

– reactivity DECREASES as you go down!





The Periodic Table

I VIII

1

2

3

4

Periods II III IV V VI VII<-- Group Numbers -->

•Each period relates to one ENERGY LEVEL

•All elements in a PERIOD have valence electrons in the same

ENERGY LEVEL

First Energy Level

Second Energy Level

Third Energy Level etc.





Diatomic MoleculesSome elements have atoms that ALWAYS exist in PAIRS. Two atoms of

the element bond to form a DIATOMIC MOLECULE.

In their natural (uncombined) states they are ALWAYS written as:

H2 N2 O2 F2 Cl2 Br2 I2 At2

They can exist singly in compounds:

H2 + Cl2 2HCl

Diatomic molecules single atoms in compound

IVIII

II III IV V VI VIIHN O F

Cl

Br

I

At

Hydrogen

GasH H

H x H•

H2

H Cl

H Cl





The Periodic TableColumns - Groups - 8

Non-metals

metals

semi-metalsHalogensI

II III IV V VI VII

Rows - Periods

Nobel/Inert

Gases





Hi -

This is a SAMPLE presentation only.

My FULL presentations, which contain a lot more more slides and other resources, are freely

available on my resource sharing website:

www.warnescience.net(click on link or logo)

Have a look and enjoy!

WarneScience






Education

Atomic Structure Revision