Download Unit 3 Powerpoint

The
Periodic
Table
A. Mendeleev

Dmitri Mendeleev (1869, Russian)
◦ Organized elements
by increasing
atomic mass.
◦ Elements with
similar properties
were grouped
together.
◦ There were some
discrepancies.
C. Johannesson
A. Mendeleev

Dmitri Mendeleev (1869, Russian)
◦ Predicted properties of undiscovered
elements.
C. Johannesson

Henry Moseley (1913, British)
◦ Organized elements by increasing atomic
number.
◦ Resolved discrepancies in Mendeleev’s
arrangement.
B. Moseley
C. Johannesson
II. Organization
of the
Elements
https://www.youtube.com/watch?v=
VgVQKCcfwnU
A. Metallic Character



Metals
Nonmetals
Metalloids
C. Johannesson
B. Blocks
Main Group
Elements
 Transition Metals
 Inner Transition
Metals

C. Johannesson
Do Now:

Classify the following as either a
METAL, NON-METAL or METALLOID:
a.Au
b.Si
c. Br
d.O
e.F
f. H
Periods and Families

Periods: horizontal rows on the
periodic table
◦ physical and chemical properties change
somewhat regularly across a row.
◦ Elements closer to each other in the same
period tend to be similar than those that
are farther apart.

Families: vertical rows of elements,
aka groups
◦ Each group contains similar chemical
properties
Types of Elements
 METALS:

Shiny

Conductors of heat and electricity

Most metals are malleable (can be
pounded into thin sheets; a sugar cube
sized chunk of gold can be pounded into a
thin sheet which will cover a football field),

Most metals are ductile (can be drawn out
into a thin wire).
Metals cont…..





All are solids at room temp (except
Mercury, which is a liquid)
Metals tend to have low ionization
energies, and typically lose electrons
(i.e. are oxidized) when they
undergo chemical reactions
Alkali metals are always 1+ (lose the
electron in s subshell)
Alkaline earth metals are always 2+
(lose both electrons in s subshell)
Compounds of metals with nonmetals tend to be ionic in nature.
Types of Elements
 NON- METALS:
Vary greatly in appearance
Non-lustrous
Poor conductors of heat and electricity
The melting points of non-metals are
generally lower than metals
 Seven non-metals exist under standard
conditions as diatomic molecules:
H2(g) N2(g) O2(g) F2(g) Cl2(g) Br2(l)
I2(l) (volatile liquid - evaporates readily)





Nonmetals, when reacting with metals,
tend to gain electrons (typically attaining
noble gas electron configuration) and
become anions: Nonmetal + Metal -> Salt

Compounds composed entirely of
nonmetals are molecular substances (not
ionic)
Non-Metals cont……..
Types of Elements

Metalloids:

Elements may share properties of metals
and non-metals.

A stair-step line separates the metals
from the nonmetals on the periodic
table.
Metalloids cont……
Properties:
 All metalloids are solids at room
temperature.


Less malleable than metals but not as brittle
as nonmetals.

Metalloids tend to be semiconductors of
electricity. (intermediate between metals and
nonmetals).
Metalloids cont……

Properties:

Metalloids are used in semiconducting
materials found in computers,
calculators, televisions and radios.

Elements include: boron, silicon,
germanium, antimony
Noble Gases
Noble Gases - the elements in Group 18
of the periodic table.
 They are considered nonmetals.
 These elements are generally unreactive.
 All are gases at room temperature.
 Examples: neon, argon, krypton, xenon
(all used in lighting) and helium.

Do Now:

Classify the following as either a
METAL, NON-METAL or METALLOID:
a.An
element that is brittle and conducts
electricity
b.An element that is malleable
c. An element that has tendency to
become an anion
ATOMIC STRUCTURE
DO NOW:
Match the scientists with the
description.
1. Came up the plum pudding model.
A. Modern Scientists
2. Came up the word atom from
”atomos”
B. Thompson
3. Discovered the positive nucleus and
the atom is mostly empty space.
C. Bohr
4. Discovered the electrons travel in
energy level (orbitals)
D. Democritus
5. Came up the idea of electron clouds
instead of orbitals.
E. Rutherford
History – ancient Greeks
Democritus – (460-370 B.C.)
• Matter is composed of atoms – moving around in empty space
• Atoms are solid homogeneous, indestructible and indivisible
• Different size and shape
• Size shape & movement determine the properties of matter
Aristotle – ( 384 322 B.C.)
• Empty space cannot exist
• Matter is made of earth, fire air and water
https://www.youtube.com/watch?v=t
hnDxFdkzZs
Daltons Atomic Theory
•
•
•
•
•
•
•
John Dalton (1766-1844)
Matter is composed of extremely small particles called atoms
Atoms are indivisible and indestructible
Atoms of a given element are identical in size, mass and chemical properties
Atoms of a specific elements are different from those of another element
Different atoms combine in simple whole number ratios to form compounds
In a chemical reaction, atoms are separated, combined and rearranged
History – ancient Greeks
Give handout of History of the atom
Democritus – (460-370 B.C.)
• Matter is composed of atoms – moving around in empty space
• Atoms are solid homogeneous, indestructible and indivisible
• Different size and shape
• Size shape & movement determine the properties of matter
Aristotle – ( 384 322 B.C.)
• Empty space cannot exist
• Matter is made of earth, fire air and water
Daltons Atomic Theory
•
John Dalton (1766-1844)
•
•
•
Matter is composed of atoms
Atoms are indivisible and indestructible
Atoms of a given element are identical in size, mass and
chemical properties
Atoms of a specific elements are different from those of
another element
Different atoms combine in simple whole number ratios to
form compounds
In a chemical reaction, atoms are separated, combined and
rearranged
•
•
•
J.J. Thomson
Cathode Ray Experiment
http://www.youtube.com/watch?v=XU8nMKkzbT8
Background
Born in Manchester, England in December
1856
 Studied physics and mathematics
 Won a nobel prize in 1906

Experiment Observations
1.
An object placed between the cathode and
the opposite end of the tube cast a shadow
on the glass.
2.
A paddle wheel placed on rails between the
electrodes rolled along the rails from the
cathode toward the anode.
3.
Cathode rays were deflected by a magnetic
field in the same manner as a wire carrying
electric current, which was known to have
a negative charge.
4.
The rays were deflected away from a
negatively charged object.
Discovery of Electrons-1897
Experiments supported hypothesis that the
particles that compose cathode rays are
negatively charged
 Measured the ratio of cathode-ray particles
to their mass—found it was always the
same
 Concluded that all cathode rays are
composed of identical negatively charged
particles called electrons
 Experiments revealed the electron has a
very large charge for its tiny mass

Lord Rutherford of
Nelson
As flawlessly explained by: Adam, Jane, Justin, Jeremy,
rob
Rutherford - History




Born 1871 in New
Zealand
In early work,
discovered
radioactive half-life
Had an element
named after himrutherfordium
Became known as the
father of nuclear
physics



Assistants - Geiger and
Marsden bombarded a
thin piece of gold foil
with a narrow beam of
alpha particles.
Some of the particles were
redirected by the gold foil
back towards their source.
Rutherford thus concluded
that the force must be
caused by a very densely
packed bundle of matter with
a positive charge, which he
called the nucleus.
Discovery of the Atomic
Nucleus
The Experiment

Rutherford had discovered that the volume of the nucleus
was very small compared to the total volume of the atom,
suggesting that there was a lot of empty space.
What is an Atom?
•
The smallest particle of an element that retains the properties of an element
consists of
PROTONS
• NEUTRONS
• ELECTRONS
•
Think – Pair - Share
1. What are the three types of subatomic particles?
2. What charge does each of them have?
3. Where is each one located?
Parts of the Atom
ProtonIn nucleus, positive charge and a mass of 1 amu
NeutronIn nucleus, neutral charge and a mass of 1 amu
ElectronOutside nucleus, negative charge
and no mass
How do Atoms Differ?
•
The number of Protons identifies it as an atom of a particular element
•
Atoms are Neutral so the number of Protons (P) Equals
the number of Electron (E) or P = E
How do Atoms differ cont…
•
Atomic Number = The number of Protons
= The number of Electrons
Mass Number is the Atomic Number (Protons)
PLUS number of Neutrons (NOT on the
Periodic Table!)
Mass Number = P + N
THINK – PAIR - SHARE
1. Identify the atomic numbers for the following elements.
A. He
B. Be
C. Ti
D. F
E. O
2. How many protons and how many electrons does
fluorine have?
How do Atoms differ cont…
Every neutral (uncharged) atoms contains an equal number of
positively charged protons (+) and negatively charged (-) electrons.
# of (+) protons = # of (-) electrons
Positive-Negative attractions between the protons in one atoms the electrons
in another atom hold atoms together in bonds.
DO NOW:
Element Name
Atomic Number
Mass Number
# of Protons
Au
# of Neutrons
12
Na
W
# of Electron
184
197
Take out your homework!
Objectives…
1. SWBAT to determine proton, neutron, electron number of given atoms.
2. SWBAT define isotope and practice writing atoms in isotopic notation.
3. SWBAT work with a partner to start to review for their upcoming quiz.
ISOTOPES
Isotopes - Atoms of the same element have same
number of protons BUT different
number of Neutron
EX:
Copper has two isotopes :
Cu 29 protons & 34 Neutrons (Cu - 63)
Cu 29 Protons & 36 Neutrons (Cu - 65)
https://www.youtube.com/watch?v=GsJPxR6IfZI
Isotopes

Atoms of the same element with different mass numbers.
 Nuclear symbol:
Mass #
12
6
Atomic
#
 Hyphen notation: carbon-12
C
Isotopes
© Addison-Wesley Publishing Company, Inc.
Do Now: Complete the chart
Part of Atom
Charge
Mass
Proton
Neutron
Electron
Take out your homework!
Location
Do Now:
How many protons, neutrons, and electrons do the
following examples contain?
5. ELECTRONS
Lets Look at ELECTRONS
•
•
•
•
Found orbiting outside of the nucleus
Electrons found at different energy levels
Outer most electrons are called Valence Electron
Valence Electrons determine the chemical properties
of an element
Lewis Dot Structure
Valence Electrons: outermost electrons
Electron Configuration:
Energy Level
MAX. # of electrons
1st
2
2nd
8
3rd
8
4th
8
Determining approximate placement of electrons
Energy Level
MAX. # of electrons
1st
2nd
3rd
4th
Chlorine (atomic #_____)
 # protons = _____
 # electrons = _____

WORKSHEET
Outermost energy level: _________
# of valence electrons: __________
Isotopes

Atoms of the same element with different mass numbers.
 Nuclear symbol:
Mass #
12
6
Atomic
#
 Hyphen notation: carbon-12
C
Do Now

Draw out the entire atom for: Boron (B)

Atomic Mass: 11
DO NOW
Energy Level
MAX. # of electrons
1st
2nd
3rd
4th
Oxygen (atomic #_____)
 # protons = _____
 # electrons = _____

TAKE OUT YOUR HOMEWORK!!!!!!!!!
Outermost energy level: _________
# of valence electrons: __________
DO NOW:

Element X has three naturally occurring
isotopes. The mass (amu) and %
abundance of the isotopes are 37.919
amu (5.07%), 39.017 amu (15.35%),
and 42.111 amu (79.58%). What is
the average atomic mass of element X?
Lewis Dot Structure:
Practice:
Draw the Lewis Dot Diagrams for the following Atoms:

Ca

Li
F
 Worksheet: Lewis Dot Diagrams

Do Now:
Draw the Lewis Dot Diagrams for the following Atoms:
 Ar

K

S

Take out your homework.
Unit 4 . IONS
https://www.youtube.com/watch?v=
900dXBWgx3Y
Ions and Ionic Compounds
 Recall:
Molecules make up one kind of Molecular
compound.
 Ions make up another kind of compound- called Ionic
Compound
61
IONS cont……
• Ions are electrically charged atoms (or groups of atoms).
• Ions are formed when neutral atoms gain or lose Valence
electrons.

List the number of protons, electrons, and neutrons in
Do Now
◦ 1. What is an ion?
◦ 2. What is a cation?
◦ 3. What is an anion?
◦ 4. Is the following a cation, anion, or neutral atom?
O2-

SW

1. SWBAT identify cations and anions.

2. SWBAT calculate the number of protons, neutrons,
and electrons in different ions.

3. SWBAT to predict the ion the atom will most likely
form.
Objectives
Ions
◦ Recall: What charge do electrons carry?
 Negative
◦ When atoms gain negative electrons, they form negative ions.
◦ When atoms lose negative electrons, they form positive ions.
65
Ions

For example, sodium (Na) is # 11 on the Periodic Table.

It has 11 (+) protons and 11 (-) electrons.

If it lost 1 (-) electron, it would have 11 (+) protons and 10 (-)
electrons.

It has one more proton than electrons, so it has a charge of +1.

The symbol for a sodium ion is Na1+ or just Na+. (The 1 is
understood.)
66
Ions
◦ For another example, chlorine (Cl) is # 17 on the Periodic Table.
◦ It has 17 (+) protons and 17 (-) electrons.
◦ If it gained 1 (-) electron, it would have 17 (+) protons and 18 (-)
electrons.
◦ It has one less proton than electrons, so it has a charge of -1.
◦ The symbol for a chloride ion is Cl1- or just Cl-. (The 1 is
understood.)
67
Think – Pair- Share
◦ Identify the number of protons and neutrons for the following
examples.
◦ 1. Si2p= ______ n= __14____ e= ______
◦ 2. Na+
p= ______ n= __12____ e= ______
◦ 3. F◦ p= ______ n= __10____ e= ______

Do any of these atoms have complete valence shells?

List the number of protons, electrons, and neutrons in
Do Now
◦ 1. What charge do elements in group 2 get?
◦ 2. What charge do elements in group 16 get?
◦ 3. What charge do elements in group 18 get?
◦ 4. Cations tend to be metal or nonmetals???
◦ 5. Anions tend to be metal or nonmetals???

List the number of protons, electrons, and neutrons in
Do Now
◦ 1. What charge does Li get when it becomes an ion?
◦ 2. Is it a cation or anion?
◦ 3. What charge does O get when it becomes an ion?
◦ 4. Is it a cation or anion?

List the number of protons, electrons, and neutrons in
Do Now
◦ 1. What is the name for NaCl?
◦ 2. Which is the cation?
◦ 3. Which is the anion?
Take out your review sheet.

SW

BAT determine the formulas for ionic compounds

SWBAT name different ionic compounds
Objectives
https://www.youtube.com/watch?v=zpaHPXVR8WU
Ionic Compounds
 Oppositely charged ions connect together to form ionic
compounds.
 For example, sodium ions (Na+) connect to chloride ions (Cl-)
to make sodium chloride
(NaCl), or table salt.
73
Sodium chloride consists of an equal number of
positive and negative ions arranged in a 3dimensional network called a crystal.
A scanning electron micrograph shows the cubic
structure of NaCl crystals.
74
A space-filling model of Nacl provides
information about how the individual sodium
ions & chloride ions are arranged within the
salt crystal.
What else does this model suggest about the
sodium and chloride ions or sodium
chloride?
75
If an ionic compound dissolves in water, the individual
ions would separate from each other and spread out
throughout the water.
To show that they were now in an aqueous solution, an
(aq) would be added after the symbols for the ions.
Na+(aq) Cl- (aq)
76
More about Ions
Cation – positive ion

Na+,
Anion – negative ion

Cl-

Monoatomic ions (or monatomic)

Na+, Cl-, Mg2+, O2-, Al3+, N3-

Polyatomic ions

NH4+, CO32-, SO42-, PO43-


77
Common Ions
 See text p. 40 for a list
of common ions.
78
Formulas for Ionic Compounds

3 Rules for Writing Formulas for Ionic Compounds

1. Cation first, then anion

2. Correct formula will be neutral, with the fewest number of each ion needed to make
the total electrical charge zero

3. No charges are shown in the formula.
79
Practice Problems


NaCl
◦ One Na1+ and one Cl1- cancel each other out.
 +1 + -1 = 0
CaCl2
◦ One Ca2+ needs two of the Cl1- to cancel it out.
 +2 + -1 + -1 = 0
Note: Negative monoatomic ions
change their ending to “ide.”
Examples above are sodium chloride
and calcium chloride.
Formulas Containing Polyatomic Ions

Formulas for compounds containing polyatomic ions follow the same
rules

If a subscript is needed, it follows the entire polyatomic ion, which is
enclosed in parentheses

For example, the calcium ion has a +2 charge, and the nitrate ion has a 1 charge
81
Formulas Containing Polyatomic Ions
For example, the calcium ion has a +2 charge (Ca2+),
 and the nitrate ion has a -1 charge (NO31+).


Two nitrate ions are needed to balance out the charge on one calcium
ion.

The formula for calcium nitrate is: Ca(NO3)2.
No charges are shown in the formula.

Polyatomic ions do not change their endings.
82

Find trends on the periodic table
Practice:

Work

Worksheet on writing ionic compounds

List the number of protons, electrons, and neutrons in
Do Now
◦
◦
◦
◦
1. What is an ion?
2. What is a polyatomic ion? Monoatomic ion?
3. What is an ionic compound?
4. What type of “bond” holds an ionic compound together?
DO NOW:

Write the formula and name the following ionic compounds


1. Ca2+
2. PO433. CO324. Al3+

What does the word “ionic” mean?


BrAg+
NH4+
NO3-
Try THESE!

Write the formula following ionic compounds
1. Lithium and Oxygen
2. Calcium and Hydroxide
3. Ammonium and Phosphate
Naming Ionic Compounds
https://www.youtube.com/watch?v=vfYnhnfdsD0

1. Name the cation, then the anion

2. Have the last few letters changed to –ide (monoatomic ions only)

Ex. KF, potassium fluoride

Ex. Ca(NO3)2, calcium nitrate

Practice Worksheet Unit 1B.9 & B.10 Ion supplement
TRY THIS…

Write the formula and name the following ionic compounds


1. Ca2+
2. PO433. CO324. Al3+

What does the word “ionic” mean?


BrAg+
NH4+
NO3-
Do Now

Write the name for following ionic compounds
1. K2S
2. B2(SO3)3
3. NH4Cl
 Worksheet (Unit 1B.9 part 3)
Practice:
 Study for quiz
◦
◦
◦
◦
What are ions? Polyatomic ions? Monoatomic ions?
How do you find the charge on a monoatomic ion?
What is an ionic compound? Ionic bond?
Writing formulas for ionic compounds. Where does the cation
go? Anion?
◦ Writing names for ionic compounds.