Download Bohr Model (Day 3) File - Galena Park ISD Moodle

S.MORRIS 2006
Warm Up
Assignment#3 1/6/17
1. What is an atom?
2. Is Na (Sodium) a Metal, Non-Metal, or a Metalloid?
3. Is Si (silicone) a Metal, Non-Metal, or a Metalloid?
4. Which of the following is dull?
Titanium Ti
Carbon C
Iron
Fe
Study for your quiz on density word problems
Bohr Model Video
HISTORY OF THE ATOM
1913
Niels Bohr
studied under Rutherford at the Victoria
University in Manchester.
Bohr refined Rutherford's idea by adding
that the electrons were in orbits.
Bohr’s Atom
electrons are
located in
orbits outside
the nucleus.
nucleus
Electron
Cloud: all the
area outside
the nucleus
HELIUM ATOM
-Orbit
-Shell
proton
-Energy
level
+
-
N
N
+
-
electron
Protons and Neutrons are
located inside the nucleus
neutron
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
HELIUM ATOM
-Orbit
-Shell
proton
-Energy
level
+
-
N
N
+
nucleus
neutron
electron
Draw the Atom
ATOMIC STRUCTURE
2
He
4
3rd
Atomic number
the number of
protons and/or
electrons in an atom
Atomic mass
the sum of protons and
neutrons in an atom
Period, put this in your notes,
continue last assignment, draw the
square around He
Find the number of electrons and protons in each one
of the following elements:
+Protons
Ex: Hydrogen
1
Fluorine
Nitrogen
Boron
Chlorine
Sulfur
Sodium
Beryllium
Carbon
Helium
Argon
Selenium
-Electrons
1
1.Where is an electron? Charge?
2.Where is a Proton? Charge?
3.Where is a Neutron? Charge?
4.What is the name of the area outside the
nucleus?
5.Which subatomic particle has the least amount
of mass?
6.Which two subatomic particles make up most
of the weight of an atom?
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
ATOMIC STRUCTURE
There are two ways to represent the atomic
structure of an element or compound;
1.
2.
Electronic Configuration
Dot & Cross Diagrams
ELECTRONIC CONFIGURATION
With electronic configuration elements are represented
numerically by the number of electrons in their shells
and number of shells. For example;
Nitrogen
2 in 1st shell
5 in
2nd
shell
configuration = 2 , 5
2
+
5 = 7
N
7
14
1. ELECTRONIC CONFIGURATION
Write the electronic configuration for the following
elements;
a)
Ca
20
b)
Na
40
2,8,8,2
d)
Cl
17
35
2,8,7
11
23
c)
2,8,1
e)
Si
14
28
2,8,4
O
8
16
2,6
f)
B
5
11
2,3
Warm up 1/9/17
Assignment #4
Draw and label the following parts of the atom
DOT & CROSS DIAGRAMS
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
X X
N
XX
X X
N
7
14
2. DOT & CROSS DIAGRAMS
Draw the Dot & Cross diagrams for the following
elements;
X
8
17
X
a) O
b)
Cl 35 X
16
X
X
X
X
X
X
X X X Cl X X
X
X
X
O
X
X
X
X
X
X
X
X
X
Valence Electrons
Valence Electrons
Electrons located in the outer
shell of an atom; responsible for
interactions with other elements
(reactions).
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-
SUMMARY
1. The Atomic Number of an atom = number of
protons in the nucleus.
2. The Atomic Mass of an atom = number of
Protons + Neutrons in the nucleus.
3.
The number of Protons = Number of Electrons.
4.
Electrons orbit the nucleus in shells.
5.
Each shell can only carry a set number of electrons.
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?
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
Mg (Magnesium)
Cr (Chromium)
S (Sulfur)
Ne (Neon)
Cl (Chloride)
Na (Sodium)
Li (Lithium)
# of Protons
# of Electrons
Overall Charge
Atomic Number
Protons
Same
Number
every time.
Electrons
Mass (Atomic Mass)
Atomic Number
Neutrons
Lets Practice “aPe”
Who am I? I have:
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
Element’s name
---Do you see an element showing more than
Once?
---Which one/ones?
---Why?
Lets Practice “aPe”
Who am I? I have:
13 Protons
Element
Al (Aluminum)
8 Electrons
21 is my atomic number
52 Protons
O (Oxygen)
Sc (Scandium)
Te (Tellurium)
13 Electrons
20 is my atomic number
33 Electrons
8 Protons
Al (Aluminum)
Ca (Calcium)
As (Arsenic)
O (Oxygen)
13 is my atomic number
21 electrons
Al (Aluminum)
Sc (Scandium)
#
*
%
@
+
=
Lets Practice “Man”
Element
S
Atomic MASS
Atomic Number
Sulfur
Ca Calcium
C Carbon
Li Lithium
As Arsenic
Cl
Chlorine
Na Sodium
Mass (Atomic Mass)
Atomic Number
Neutrons
Neutrons
Warm Up
1/17/17 (Tuesday) Assign. #6
Copy the chart and fill in the blanks
Element
# of
Protons
# of
Atomic
Electrons mass
16
16
23
20
# of
Neutrons
Periodic Table
H
Li
Periods are horizontal and
determine the number of
energy levels in an atom.
Na
Periods=Rows=# OF SHELLS
Rb
K
Cs
Fr
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
Groups are vertical and determine
the number of valence electrons.
1=1
2=2
13=3
14=4
FOR COLUMNS 3-12
15=5
YOU NEED TO DO THE
16=6
ELECTRONIC
17=7
CONFIGURATION
18=8
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
Elements in the same group
have similar chemical and
physical properties.
Li
Be
S
He
Na
Mg
Se
Ne
Which one/ones have similar
Physical and Chemical
properties?
Li
Be
O
He
Mg
Sr
F
Xe
REACTIVITY
•Most reactive groups 1 & 17
•Least reactive/stable group
18
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.
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
7.Atoms of the same element with different
amounts of neutrons are isotopes.
Ex: diamond.