1. ATOMIC STRUCTURE
S.MORRIS 2006

2. Warm Up Assignment#3 1/6/17 1. What is an atom?
2. Is Na (Sodium) a Metal, Non-Metal, or a Metalloid?
Is Si (silicone) a Metal, Non-Metal, or a Metalloid?
Which of the following is dull?
Titanium Ti
Carbon C
Iron Fe
Study for your quiz on density word problems

3. Bohr Model Video

4. HISTORY OF THE ATOM Niels Bohr 1913
studied under Rutherford at the Victoria University in Manchester.
Bohr refined Rutherford's idea by adding that the electrons were in orbits.

5. electrons are located in orbits outside the nucleus.
Bohr’s Atom
electrons are located in orbits outside the nucleus.
Electron Cloud: all the area outside the nucleus
nucleus

6. Protons and Neutrons are located inside the nucleus
HELIUM ATOM
-Orbit
-Shell
-Energy level
proton N + - + N -
neutron
electron
Protons and Neutrons are located inside the nucleus

7. e- have the smallest mass (technically none). amu: Atomic mass unit
ATOMIC STRUCTURE
**********Copy and memorize the chart*************
Particle
Charge
Mass
proton
+ charge
1amu
neutron
+/-No charge
1amu
electron
- charge
0 amu
e- have the smallest mass (technically none).
amu: Atomic mass unit

8. Draw the Atom HELIUM ATOM + - + - -Orbit -Shell -Energy level proton
nucleus
neutron
electron
Draw the Atom

9. ATOMIC STRUCTURE 2
Atomic number He
the number of protons and/or electrons in an atom
Atomic mass 4
the sum of protons and
neutrons in an atom
3rd Period, put this in your notes, continue last assignment, draw the square around He

10. +Protons -Electrons Ex: Hydrogen 1 1
Find the number of electrons and protons in each one of the following elements:
+Protons -Electrons
Ex: Hydrogen
Fluorine
Nitrogen
Boron
Chlorine
Sulfur
Sodium
Beryllium
Carbon
Helium
Argon
Selenium

11. Where is an electron? Charge?
Where is a Proton? Charge?
Where is a Neutron? Charge?
What is the name of the area outside the nucleus?
Which subatomic particle has the least amount of mass?
Which two subatomic particles make up most of the weight of an atom?

12. ATOMIC STRUCTURE
Electrons are arranged in Energy Levels, Shells, or orbitals around the nucleus of an atom.
first shell a maximum of 2 electrons
second shell a maximum of 8 electrons
third shell a maximum of 8 electrons
fourth shell a maximum of 8 electrons

13. 1. Electronic Configuration
ATOMIC STRUCTURE
There are two ways to represent the atomic structure of an element or compound;
1. Electronic Configuration
2. Dot & Cross Diagrams

14. ELECTRONIC CONFIGURATION
With electronic configuration elements are represented numerically by the number of electrons in their shells and number of shells. For example;
Nitrogen
configuration = 2 , 5 7
2 in 1st shell
5 in 2nd shell N
= 7 14

15. 1. ELECTRONIC CONFIGURATION
Write the electronic configuration for the following elements; 20 11 8 Na O Ca a) b) c) 16 23 40
2,8,8,2
2,8,1
2,6 17 14 5 Cl Si B d) e) f) 11 35 28
2,8,7
2,8,4
2,3

16. Draw and label the following parts of the atom
Warm up 1/9/17
Assignment #4
Draw and label the following parts of the atom

17. N DOT & CROSS DIAGRAMS Nitrogen
With Dot & Cross diagrams elements and compounds are represented by Dots or Crosses to show electrons, and circles to show the shells. For example; X
Nitrogen N 7 X X N X X 14 X X

18. Valence Electrons 2. DOT & CROSS DIAGRAMS O Cl
Draw the Dot & Cross diagrams for the following elements; X 8 17 X O Cl a) b) X 35 X 16 X X X X X Cl X X X X X X X O X X X X X X X X X X
Valence Electrons

19. Valence Electrons
Electrons located in the outer shell of an atom; responsible for interactions with other elements (reactions).

20. Draw the Bohr Model of the first 26 elements in the periodic table, and write down the following details:
Protons#
Electrons#
Valence electrons# 1P
Valence. e=1 and 1 e-

21. SUMMARY The Atomic Number of an atom = number of
protons in the nucleus.
The Atomic Mass of an atom = number of
Protons + Neutrons in the nucleus.
The number of Protons = Number of Electrons.
Electrons orbit the nucleus in shells.
Each shell can only carry a set number of electrons.

22. WARM UP 1/12/17
Assignment # 5
1. Do the electronic configuration of the following atoms and classify them as Malleable, or
Non-Malleable
--V (Vanadium)
--S (Sulfur)
--Fe (Iron)
2. Which subatomic particles are responsible for the Atom’s weight?
3. Location of a Neutron?

23. Atoms presented in the periodic table are electrically neutral; therefore, they have the same amount of protons and electrons (They cancel each other out).
Element
# of Protons
# of Electrons
Overall Charge
Mg (Magnesium)
Cr (Chromium)
S (Sulfur)
Ne (Neon)
Cl (Chloride)
Na (Sodium)
Li (Lithium)

24. } APE MAN Same Number every time. Protons Electrons Mass (Atomic Mass)
Atomic Number
Same Number every time.
Protons
Electrons
MAN
Mass (Atomic Mass)
Atomic Number
Neutrons

25. Lets Practice “APE” Who am I? I have: 13 Protons 8 Electrons
Element’s name
13 Protons
8 Electrons
21 is my atomic number
52 Protons
13 Electrons
20 is my atomic number
33 Electrons
8 Protons
13 is my atomic number
21 electrons

26. ---Do you see an element showing more than Once?
---Which one/ones?
---Why?

27. # * Lets Practice “APE” Who am I? I have: Element 13 Protons
Al (Aluminum)
8 Electrons
O (Oxygen)
21 is my atomic number
Sc (Scandium)
52 Protons
Te (Tellurium)
13 Electrons
Al (Aluminum)
20 is my atomic number
Ca (Calcium)
33 Electrons
As (Arsenic)
8 Protons
13 is my atomic number
21 electrons # % @ = * +

28. MAN Lets Practice “Man” Mass (Atomic Mass) Atomic Number Neutrons
Element
Atomic MASS
Atomic Number
Neutrons
S Sulfur
Ca Calcium
C Carbon
Li Lithium
As Arsenic
Cl Chlorine
Na Sodium
MAN
Mass (Atomic Mass)
Atomic Number
Neutrons

29. Copy the chart and fill in the blanks
Warm Up
1/17/17 (Tuesday) Assign. #6
Copy the chart and fill in the blanks
Element
# of Protons
# of Electrons
Atomic mass
# of Neutrons 16 23 20

30. Periodic Table H Li
Periods are horizontal and determine the number of energy levels in an atom.
Periods=Rows=# OF SHELLS Na K Rb Cs Fr

31. Find the number of shells in the following elements:
1. V
2. Ge
3. F
4. H
5. He
6. As
7. Rn
8. Ne
9. S
10.K

32. Groups are vertical and determine the number of valence electrons.
1=1
2=2
13=3
14=4
15=5
16=6
17=7
18=8
FOR COLUMNS 3-12 YOU NEED TO DO THE ELECTRONIC CONFIGURATION

33. Determine the number of Valence electrons of the following Elements:
1. Mg
2. B
3. Sc
4. Be
5. Cr
6. Kr
7. Xe
8. Te
9. S
10.Si

34. Elements in the same group have similar chemical and physical properties.Li Be S He Na Mg Se Ne

35. Which one/ones have similar Physical and Chemical properties?Li Be O He Mg Sr F Xe

36. REACTIVITY
Most reactive groups 1 & 17
Least reactive/stable group 18

37. For metals, reactivity increases down a group and from right to left across a period.
For nonmetals, reactivity increases up a group and from left to right across a period.
Francium is the most reactive metal, and fluorine is the most reactive nonmetal.

38. Find the most reactive Element
1. Ne or F
2. S or Xe
3. Rb or Na
4. Ba or Mg
5. Sc or K
6. Rn or C
7. Cu or Cs
8. H or Fr
9. K or Ne
10. He or Be

39. 7.Atoms of the same element with different amounts of neutrons are isotopes.
Ex: diamond.