chapter 5 atoms & periodic table · chapter 5 atoms & periodic table 4 j.j. thomson -1856-1940...

Chapter 5 Atoms & Periodic Table

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Chapter 5 p. 166The Periodic Table

Organizes Elements by Patterns in Properties and

Atomic Structure.

Section 5.1: Developing the Atomic Theory p. 168


Atoms• All matter is formed from

small particles called atoms.

• These different atoms cause substances to have different properties!

• Humans are mostly made of oxygen, carbon, hydrogen, and nitrogen atoms.

• Can you think of other types of atoms that are part of our bodies?

• Atoms are the smallest part of an element that still have the properties of that element.


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Chemistry & Atoms Video

docx

https://www.youtube.com/watch?time_continue=7&v=8ypo6wGqIGY


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How Can You See An Atom? Video

Atomic theory is the study of the nature of atoms and how theycombine to form all types of matter.

• Atomic theory helps us to understand why there are different kinds of atoms.

• Models of atomic theory began in the 1800's and continued to evolve as technology developed.

Recall...

Section 5.1: Atomic Theory p. 171-174

Use the chart provided to create notes on each of the contributors to atomic theory (p. 171-174 in your text).

John Dalton - early 1800's• atoms were like small spheres• atoms might vary in size, mass, or color• Dalton used the particle theory to

explain the nature of matter• He devised a set of element symbols

https://www.youtube.com/watch?time_continue=3&v=ipzFnGRfsfE


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J.J. Thomson -1856-1940 • atoms are made from a combination of particles• experimented with electric currents in glass tubes (cathode ray tubes).• he caused atoms to produce streams of negatively charged particles (later called electrons).• 1897- An atom was a positive sphere with negative electrons scattered throughout.

Ernest Rutherford - (1891-1937)• tested Thomson's model• Shot positively charged particles at a very thin foil of pure gold (used a radioactive substance in a lead block with a tiny hole)• Most particles went right through, but about 1 in 10,000 bounced back as if it hit something large and positively charged.• DISCOVERY OF THE NUCLEUS - the center of the atom!

• All atoms have a nucleus which is most of the atom's mass. • Size of nucleus compared to the rest of atom like green pea on a football field.

Neils Bohr- (1885-1962) • Transformed Rutherford's model into the Bohr Diagram which is still used today.• Electrons surround the nucleus in specific energy levels called shells. • Each shell can only contain a specific number of electrons. • First shell can contain 2 electrons, second shell 8, third shell 8.• Many people still use this model to describe atoms.

Quantum Mechanical Model - • The most current model - used today by physicists and chemists.• Electrons do not exist as tiny points inside an atom. • Electrons surround the positive nucleus in a cloud.


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Bill Nye: Atoms & Molecules

Section 5.2: p. 178The Elements

https://www.youtube.com/watch?v=dDSFu1Jagbohttps://www.youtube.com/watch?time_continue=1&v=VgVQKCcfwnU


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Elements & Their Symbols p. 180

• Approximately 90 elements naturally occur on Earth

• Recently, scientists have since created more than 25 new elements.

• Based on their properties, all elements can be divided into 3 categories:> Metals> Nonmetals> Metalloids


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https://www.youtube.com/watch?time_continue=11&v=mtg9p6A6xnY


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http://www.rsc.org/periodic-table

Attachments

Intro If Atoms were Peas.doc

AtomsFamilyMath.pdf

Atomic Number Practice.doc.pdf

Atomic Mass wrksheet.pdf

Atomic Structure Notes wrksheet.pdf

If Atoms were Peas

Consider the green pea. If you took 100 (102) average sized green peas they would occupy a volume of 20 cm2. A million peas (106) are just enough to fill an ordinary sized refrigerator and a billion peas (106) will fill a three bed-room house from the cellar to the attic. A trillion (1012) peas will fill a thousand houses, about the number of houses in Souris and Kensington combined. A quadrillion (1015) peas will fill all the buildings in one of our larger cities such as Calgary or Ottawa which are about three times bigger than Halifax.

Obviously, if you have a lot of peas, you will soon run out of buildings so let’s look at area of provinces. Suppose there is a blizzard over Atlantic Canada, but instead of snowing snow, it snows peas. All of Newfoundland and Labrador, Nova Scotia, New Brunswick and Prince Edward Island become covered with a blanket of peas 1 meter deep. The blanket of peas drifts over roads, up against the side of houses and covers all the fields and forests. Think of flying across these provinces and looking down and the blanket of peas extending out as far as you can see. This gives you a clue to our next number. There will be in this blanket about quintillion (1018) peas.

Imagine that the blizzard is really, really bad and the peas fall all over the entire land region of the Earth – North America, South America, Africa, Europe, Australia and Asia. All the continents are covered with peas one metre deep. This global blanket of peas will contain sextillion (1021) peas. Then image that the oceans are frozen over and the blanket of peas covers the entire land and sea area of the Earth. You travel out into space among the neighboring stars and collect 250 planets the size of Earth and cover each of these with a blanket of peas one metre deep. You have a special number of peas 1026. Chemists call this number a mole and use it when working with atoms because they are so small that they have to work with this many to see them. But we have to collect more peas.

Go out into the farthest reaches of the Milky Way, and collect 250, 000 planets, each the size of the Earth. Cover each planet with a blanket of peas one metre deep. You now have a cotillion (1027) of peas… and… this is the same number of atoms that you have in your body.

Image source unknown

� Adapted from Alberta ALCHEM guide; original author unknown

SMART Notebook

The Atoms Family Name ___________________________Atomic Math Challenge

8

OOxygen

15.999

Atomic number equals the number of

_____________ or _____________

Atomic mass equals the number of

_____________ + _____________

8

O_______

15.999

Atomic # = ______

Atomic Mass = _________

# of Protons = ________

# of Neutrons = ________

# of Electrons = ________

30

___Zinc65.39

Atomic # = ______


# of Protons = ________



3

Li_______

6.941

Atomic # = ______


# of Protons = ________



14

___Silicon

28.086

Atomic # = ______


# of Protons = ________



5

B_______

10.81

Atomic # = ______


# of Protons = ________



35

___Bromine

79.904

Atomic # = ______


# of Protons = ________



16

S_______

32.06

Atomic # = ______


# of Protons = ________



53

____Iodine126.905

Atomic # = ______


# of Protons = ________



25

Mn_______

54.938

Atomic # = ______


# of Protons = ________



12

Mg_______

24.305

Atomic # = ______


# of Protons = ________



18

___Argon

39.948

Atomic # = ______


# of Protons = ________



19

K_______

39.098

Atomic # = ______


# of Protons = ________



79

___Gold196.967

Atomic # = ______


# of Protons = ________



1

H_______

1.008

Atomic # = ______


# of Protons = ________



9

___Fluorine

18.998

Atomic # = ______


# of Protons = ________



SMART Notebook

Name: ______________________

Date: ____________ Period:_____

Fill in all the information for each element.

Elem

ent

Sym

bol

Ato

mic

N

umbe

r

Ato

mic

W

eigh

t

Num

ber

of p

+

(pro

tons

)

Num

ber

of e

-

(ele

ctro

ns)

Num

ber

of n

0

(neu

tron

s)

Hydrogen

Fluorine

Boron

Chlorine

Aluminum

Sodium

Argon

Carbon

Helium

Oxygen

Nitrogen

Lithium

Neon

Atomic Number Practice

SMART Notebook

Atomic Mass

Name:

1. The diagram of this element shows that there are

a) protons

b) electrons

c) neutrons

From this information we know that

d) the atomic mass of the element is

e) the atomic number is

f) the symbol for the element is

2a) Below are diagrams of three atoms of the carbon element. Examine the subatomic

particles of these carbon atoms to see how the atoms differ.

#electrons

#protons

#neutrons

atomic mass

b) Identify which subatomic particles differ in number in the three atoms.

Atoms of the same type that vary this way are called isotopes. Use what you have

learned to define isotopes: Isotopes are atoms that have the same number of

but different numbers of and different

.

c) Isotopes are given a special type of symbol. The symbols for these three isotopes are 12C 13C 14C

Use the information in your table to deduce which symbol belongs to each atom above.

What information did you use to make this decision?

+

+

Protons

+ Neutrons

= Atomic Mass

3. Use your periodic table to complete the following table and then

answer the question at the bottom of the page. Remember that

the atomic number represents the number of protons. PNA

helps to remember how to calculate atomic mass.

What pattern do you notice in the number of protons and neutrons in each atom and their

relationship to atomic mass?

Name of Element Symbol Atomic Number

Atomic Mass

(round to nearest

whole number)

Number of Protons

Number of Neutrons

hydrogen 1 1.01

He 2

Li 3 6.94 3

beryllium 4

boron 5 10.81

C 6

nitrogen 7

8

fluorine 9

neon 10

Na 23.00

magnesium 24.31

Al 27.00

Si 14

P 31.00

S 16

chlorine 35.45

argon 40.00

SMART Notebook

Atomic Structure Notes

Name:

1. The three subatomic particles that compose the atom are the:

2. Add the following labels to the diagram: nucleus, energy level 1, energy level 2, valence electron, proton, and neutron.

3. What are two problems with models of the atom like the one shown in question 1?

4. Complete the following table.

Subatomic Particle

Symbol Location in atom Relative Charge Relative Mass

proton 1

neutron n0 in nucleus

electron 1/2000

5. Draw Bohr diagrams for the following atoms. Use these rules to help you.

Example: nitrogen – N Atomic number: 7

Bohr Diagrams

carbon – C Atomic number: 6

helium – He Atomic number: 2

potassium – K Atomic number: 19

fluorine – F Atomic number: 9

Elements are ordered on the periodic table by their atomic number which is the number of protons

An element has the same number of electrons as protons.

X can be used to represent an electron

The maximum number of electrons for each energy level in the first twenty elements is:

o 1st energy level: 2e-

o 2nd energy level: 8e-

o 3rd energy level: 8e-

o 4th energy level: up to 18e-

SMART Notebook

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chapter 5 atoms & periodic table · chapter 5 atoms & periodic table 4 j.j. thomson -1856-1940...

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