i. bohr’s model / energy levels a. def – a specific area where an electron is likely to be....

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I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e - e - e - e - e - e - e - e - e - e - e - e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e-

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Page 1: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

I. Bohr’s Model / Energy Levels

A. Def – a specific area where an electron is likely to be.

nucleus

2 electrons

8 electrons

18 electrons

32 electrons

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Page 2: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

Chapter 4Lesson 2

“A Tour of the Periodic Table”

Page 3: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

I. Organization of the P.T.

A. Periodic Law1. Def – Elements are arranged according

to properties.2. Ex: Group 1 Elements Video3. Periods – horizontal4. Group – Vertical

a. Aka family

Page 4: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

Page 5: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

II. Ions

A. Def – an atom that gains or loses electrons. Will have a negative or positive charge.

B. Ex: Fluorine (pg. 115)

F2e7e

e

8e

What kind of charge willfluorine have now as an ion?

1-

Page 6: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

III. Atomic Number

A. Def – the # of protons in an atom’s nucleus.

B. On P.T. – located right above the chemical symbol

*Protons dictate the type of element we have**Electrons always equal the # of protons in a

neutral atom*

Page 7: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

IV. Mass Number

A. Def – The sum of protons and neutrons in the nucleus of an atom.1. On P.T. – bottom number

-round up/down2. Ex: What is the mass number of the following elements?

Carbon OxygenIron CalciumSodium Zinc

12

56

23

16

40

65

Page 8: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

3. Mass # = Protons + Neutrons

4. How many Neutrons on average are found in the following elements?Boron FluorineSilicon CopperSilver Gold 118

14

6

61

10

35

Page 9: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

V. Isotope

A. Def – An atom that has a different number of neutrons.1. Does not affect the element2. Only changes the weight of the element

3. Ex: Boron-10 and Boron-11

p p p p p p p p p p

n n n n nn n n n n n

5 protons 5 protons

5 neutrons 6 neutrons

This meansthe mass #

Boron-10 Boron-11

Page 10: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

4. How many neutrons do the following isotopes have?

Oxygen-14Titanium-50Magnesium-22Potassium-43Aluminum-23Iodine-130

6

28

10

24

10

77

Page 11: I. Bohr’s Model / Energy Levels A. Def – a specific area where an electron is likely to be. nucleus 2 electrons 8 electrons 18 electrons 32 electrons e-e-

VI. Average Atomic MassA. Def – average mass of all isotopes of one

element combined.1. Found on P.T. underneath chemical symbol.2. Ex: Carbon = 12.011

“Carbon has 3 known isotopes. Carbon-12, 13, and 14. Carbon-12 makes up 99% of all carbon on earth. Carbon-13 and 14 make up 1%.”

Why?

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