Download The Atom and the Periodic Table

The Atom and the Periodic Table
Chapter 10 and Chapter 11
Objectives
• SPI 0807.9.1 Recognize that all matter consists
of atoms
• I can:
1. I can recognize that all matter is made of
atoms.
2. I can identify the parts of an atom.
3. I can identify the charge and location of each
particle in an atom.
4. Explain how an atom can be neutral and how
the atom can become charged.
I can recognize that all matter is made of atoms.
History of Atomic Theory
• Democritus – Greek philosopher 400 BCE
 Thought you could eventually end up with a particle that
could not be cut in half – he called this particle an atom.
 From Greek word “atomos” meaning “not able to be divided”
 Most people did not believe this to be true including
Aristotle.
 Did not perform experiments to prove theory, it was just
an idea
• Democritus was right: matter is made of
particles called atoms – the smallest particle
into which an element can be divided and
still be the same substance
I can recognize that all matter is made of atoms.
Dalton’s Atomic Theory
• John Dalton – British chemist and schoolteacher
▫ Published his theory in 1803
1. All substances are made of atoms. Atoms
are small particles that cannot be created,
divided, or destroyed.
2. Atoms of the same element are exactly
alike and atoms of different elements are
different.
3. Atoms join with other atoms to make new
substances.
I can recognize that all matter is made of atoms.
I can identify the charge and location of electrons in an atom.
Thomson’s Discovery of Electrons
• J. J. Thomson(1897) – British
scientist (awarded Nobel Prize
in 1906)
• Proved Dalton’s theory had a
mistake: atoms can be divided
into smaller parts.
▫ Discovered electrons (e-) –
subatomic particle that
has a negative charge
• Plum-pudding model
▫ Electrons were mixed
throughout an atom
I can recognize that all matter is made of atoms.
I can identify the parts of an atom.
Rutherford’s Theory
• Ernest Rutherford (1911)–
student of Thomson (awarded
Nobel Prize in 1908)
▫ Proposed that the center of
the atom is the nucleus –
tiny, extremely dense
positively charged part of
the atom
I can recognize that all matter is made of atoms.
I can identify the particles that make up an atom.
Bohr’s Model
• Niels Bohr (1913) – Danish
scientist, worked with
Rutherford (awarded Nobel
Prize in 1922)
▫ Proposed that electrons
move around the nucleus
in certain paths or energy
levels.
 Electrons can jump from one
level to another level but do
not occupy the space
between the energy levels.
I can recognize that all matter is made of atoms.
I can identify the location of each particle in an atom.
The Modern Atomic Theory
• Erwin Schrodinger – Austrian
physicist (awarded Nobel Prize
in 1933)
• Werner Heisenberg – German
physicist (awarded Nobel Prize
in 1932)
▫ Electrons travel in
regions around the
nucleus of an atom where
they are likely to be
found called electron
clouds
Democritus
Atom – smallest particle that cannot be divided
Dalton (1803)
All substances made of atoms
Atoms can join to make new substances
Thomson (1897)
Discovered electrons-negative particle
Plum-pudding model
Rutherford (1911)
Nucleus-central region of atom that has positive charge
Bohr (1913)
Energy levels-paths in which electrons travel
Modern Atomic Theory (20th century)
Schrodinger, Heisenberg
I can recognize that all matter is made of atoms.
Electron clouds-regions electrons likely found
Objectives
• SPI 0807.9.1 Recognize that all matter consists of atoms.
• SPI 0807.12.5 Determine the relationship among the mass of
objects, the distance between these objects, and the amount of
gravitational attraction.
• I can:
1. I can recognize that all matter is made of atoms.
2. I can identify the parts of an atom.
3. I can identify the charge and location of each particle in an
atom.
4. Explain how an atom can be neutral and how the atom can
become charged.
5. Explain how gravity is affected by the mass of an object and
the distance between objects.
I can recognize that all matter is made of atoms.
The Atom
• Extremely small
▫ One penny contains 2 x 1022 atoms
▫ One Al atom has a diameter of 0.00000003 cm
▫ Al foil is 50,000 atoms thick
I can identify the parts of an atom.
I can identify the charge and location of each particle in an atom.
The Atom
• Nucleus – small, dense, positively charged center of the
atom
▫ Contains most of the atom’s mass
1. Protons (p+)– positively charged particle in the
nucleus
2.
•


▫
▫
▫
Mass of one proton is 1.7 x 10-24 g = 1 amu (atomic mass unit)
Neutrons (n0)– particles in the nucleus that has no
charge.
Mass = 1 amu
Electrons – negatively charged particles of an atom
Found outside the nucleus in electron clouds
Mass of one electron is almost zero
1,800 electrons = mass of 1 proton
I can identify the parts of an atom.
I can identify the charge and location of each particle in an atom.
I can identify the parts of an atom.
I can identify the charge and location of each particle in an atom.
Explain how an atom can be neutral and how the atom can become charged.
The Atom
• # of protons = #of electrons
▫ The charges cancel out, so the atom has an overall
neutral charge
• If protons ≠ electrons, then the atom becomes
charged
▫ Ion – charged particle
▫ Lose electron → lose negative → positive ion
▫ Gain electron → gain negative → negative ion
I can explain how gravity is affected by the mass of an object and the
distance between objects.
Forces in Atoms
1. Gravitational forces
▫
▫
▫
Acts on all objects all the time
Pulls objects toward one another
Depends on mass and distance between particles


▫
Greater mass has greater gravitational pull
Closer distance has greater gravitational pull
Very small in atoms
I can explain how gravity is affected by the mass of an object
and the distance between objects.
Forces in Atoms
2.
Electromagnetic Force
▫
▫
▫
▫
Same charge repels
Opposite charges attract
Protons and electrons
attract
Holds electrons around the
nucleus
I can explain how gravity is affected by the mass of an object and
the distance between objects.
Forces in Atoms
3. Strong force
▫
▫
Holds protons together in the nucleus
Greater than EM force
I can explain how gravity is affected by the mass of an object and
the distance between objects.
Forces in Atoms
4. Weak force
▫
▫
Found in radioactive elements (unstable
atoms that spontaneously fall apart over
time)
Allows a neutron to change into a proton or
electron
Objectives
• SPI 0807.9.1 Recognize that all matter consists of
atoms.
• SPI 0807.9.9 Use the periodic table to determine the
properties of an element.
• I can:
1. Identify the parts of an atom.
2. Identify the charge and location of each particle in
an atom.
3. Identify the atomic number, atomic mass, number
of protons, neutrons, and electrons in an atom
using the periodic table.
I can identify the atomic number, atomic
mass, number of protons, neutrons, and
electrons in an atom using the periodic
table.
Building Atoms
1. Determine atomic number for the element
▫
Top number on periodic table

Number of protons and electrons for that element
2. Determine atomic mass for the element
▫
Bottom number (rounded) on periodic table
▫
Number of neutrons
▫
Only 2 electrons go in the first energy level, only 8 in the
second, 18 in the third, 32 in the fourth, 50 in the fifth, 72
in the sixth
3. Subtract atomic # from atomic mass
4. Draw the atom with the correct number of protons and
neutrons in the nucleus
5. Place electrons in electron clouds around the nucleus
I can identify the atomic number, atomic
mass, number of protons, neutrons, and
electrons in an atom using the periodic
table.
Carbon
1. Atomic number = 6
▫
# of protons = # of electrons = 6
2. Atomic mass = 12.01 =12
3. Atomic mass – atomic # = # of neutrons
▫
12 – 6 = 6 neutrons
I can identify the atomic number, atomic
mass, number of protons, neutrons, and
electrons in an atom using the periodic
table.
Aluminum
1. Atomic number = 13
▫
# of protons = # of electrons = 13
2. Atomic mass = 26.98154 =27
▫
Atomic mass – atomic # = # of neutrons
3. 27 – 13 = 14 neutrons
I can identify the atomic number, atomic
mass, number of protons, neutrons, and
electrons in an atom using the periodic
table.
Isotopes
2,670 known isotopes
38 isotopes of tin
• Atoms that have a different number of
neutrons, but the same number of
protons
▫ Isotopes are still the same element, because they
have the same number of protons
 The number of protons determine which element
you have
 If you change the # of protons, then the element
changes
▫ Isotopes have the same chemical properties and
most physical properties
I c an identify the atomic number, atomic
mass, number of protons, neutrons, and
electrons in an atom using the periodic
table.
Naming Isotopes
1. Write the name of the element
2. Followed by a hyphen (-)
3. Followed by the mass # of the isotope
•
•
•
•
Hydrogen-1
Lithium-5
Cobalt-60
Gallium-71
I c an identify the atomic number, atomic
mass, number of protons, neutrons, and
electrons in an atom using the periodic
table.
Boron
Boron-10
Boron-11
•
•
•
•
•
•
•
•
Atomic # = 5
#of protons =# of electrons = 5
Mass number = 10
Mass # - atomic # = # neutrons
▫ 10-5 = 5 neutrons
Atomic # = 5
#of protons =# of electrons = 5
Mass number = 11
Mass # - atomic # = #
neutrons
▫ 11-5 = 6 neutrons
The Periodic Table
Chapter 11
Objectives
• SPI 0807.9.9 Use the periodic table to determine the properties of an
element.
• I can:
1.
Explain how the periodic table was first arranged and how it is arranged
today.
2. Identify each element as a metal, nonmetal, or metalloid using the zigzag
line as a reference.
3. Identify an element by its chemical symbol.
4. Identify the groups and periods of the periodic table.
5. Describe how chemical properties of elements are similar in the same
group.
6. Label each group by name (ex: alkali metals, halogens, noble gases, etc.)
7. Identify similar properties for each group.
8. Explain which groups are likely to react together .
I can explain how the periodic table was first arranged and
how it is arranged today.
The Pattern
• Dmitri Mendeleev, Russian chemist
▫ Discovered pattern in 1896 (63 elements has been
discovered by this time)
 Wrote the names and properties of each element on cards
and arranged the cards by properties, density,
appearance, and melting point – no pattern
 Arranged by increasing atomic mass – pattern appeared
• Pattern was periodic – repeats at regular
intervals
▫ Mendeleev named his table the Periodic Table of
elements
▫ Mendeleev predicted properties of missing elements
not yet found
I can explain how the periodic table was first arranged and
how it is arranged today.
Germanium
Mendeleev’s
prediction
Actual Properties
Atomic mass
70
72.6
Density
5.5
5.3
Appearance
Dark gray metal
Gray metal
Melting Point
High melting point
937◦C
I can explain how the periodic table was first arranged and
how it is arranged today.
Changing the Arrangement
• Henry Moseley, British scientist
▫ 1914 - Determined the atomic number for each
element
▫ Rearranged the PT by increasing atomic number
▫ All elements follow periodic law – the
repeating chemical and physical properties
of elements change periodically with the
elements’ atomic numbers
I can explain how the periodic table was first arranged and
how it is arranged today.
I can identify each element as a metal, nonmetal, or metalloid
using the zigzag line as a reference.
Decoding the Periodic Table
1.
a.
b.
c.
Metals, Nonmetals, Metalloids
Metals













Left of zigzag line
Few electrons in outer energy level
Most are solid at RT
Shiny, malleable, ductile, good conductors of heat and electricity
Nonmetals
Right of zigzag line
Almost complete set of electrons in outer energy level
Noble gases (group 18) have complete set of electrons
Most are gases at RT
Not shiny, not malleable, not ductile, poor conductors, brittle
Metalloids
Along zigzag line
Half of a complete set of electrons in outer energy level
Semiconductors
Properties of both metals and nonmetals
I can identify each element as a metal, nonmetal, or metalloid
using the zigzag line as a reference.
I can identify an element by its chemical symbol.
Decoding the Periodic Table
2.
Chemical Symbol
▫
Names come from
scientists, places

▫
Mendelevium,
californium
Symbols are the same
worldwide
Consists of one or two
letters
▫



First letter is ALWAYS
capitalized
Second letter is ALWAYS
lowercase
Newer elements have 3
letters
I can identify an element by its chemical symbol.
I can recognize that all
matter is made of atoms.
I can identify an element by its chemical symbol.
I can identify the groups and periods of the periodic table.
Decoding the Periodic Table
3. Periods
▫
▫
▫
▫
Horizontal rows of elements (left to right)
Follow periodic pattern across a period
Becomes less metallic as you go to the right on the
PT
Seven periods
4. Groups (Family)
▫
▫
▫
Vertical columns of elements (top to bottom)
Similar chemical and physical properties
Eighteen groups
Reading the Periodic Table
1.
2.
3.
4.
5.
6.
7.
8.
9.
What information is given in each square on the periodic table?
▫
▫
▫
▫
▫
AN, AM, symbol, name, state, protons, electrons
How many elements are liquid at RT? Which ones?
2
Hg, Br
How many are gas at RT?
11
How many are metals?
88
How many are nonmetals?
▫ 18
How many are metalloids?
▫
▫
▫
6
How many groups?
18
How many periods?
7
List elements whose symbols do not seem to come from their English
names?
▫
Sn, Hg, Pb, Sb, W, K, Na
▫
S, Se, Te, Po
10. What elements are in the same group as oxygen?
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Grouping the Elements
• Properties are similar in groups
• Atoms in each group have the same number of
electrons in their outer energy level
▫ Atoms will gain, lose, or share electrons with other
atoms to obtain a complete set of electrons in their
outer energy level
▫ These atoms will form compounds
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Group 1: Alkali Metals
•
•
•
•
•
•
•
All metals
1 electron in outer energy level
Very reactive
Soft
Silver
Shiny
Low density
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Group 2: Alkaline-Earth Metals
•
•
•
•
•
Metals
2 electrons in outer energy level
Very reactive but less than alkali metals
Silver
Low density but higher than alkali metals
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Groups 3-12: Transition Metals
•
•
•
•
•
Metals
1 or 2 electrons in outer energy level
Less reactive than alkaline-earth metals
Shiny
Good conductors of thermal energy and electric
current
• Higher densities and melting points than
elements in groups 1 and 2 (except mercury)
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Lanthanides
• Period 6
• Shiny
• reactive
Actinides
• Period 7
• Radioactive
• Elements after 94 (plutonium)
are made in laboratories
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Group 13: Boron Group
•
•
•
•
•
One metalloid, 4 metals
3 electrons in OEL
Reactive
Solids at room temperature
Aluminum (Al) is the most abundant
element on Earth
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Group 14: Carbon Group
• 2 metals, one nonmetal, two metalloids
• 4 electrons in OEL
• Solids at RT
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Group 15: Nitrogen Group
•
•
•
•
1 metals, 2 metalloids, 2 nonmetals
5 electrons in OEL
Solids at RT
Nitrogen makes up to 80% of air
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Group 16: Oxygen Group
•
•
•
•
•
1 metal, 1 metalloid, 3 nonmetals
6 electrons in OEL
All solids except oxygen (gas)
Reactive
Oxygen makes up about 20% of air
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Group 17: Halogens
• Nonmetals
• 7 electrons in OEL (only need to gain 1 electron
for complete outer level)
• Very reactive
• Poor conductors of electric current
• React with alkali metals
(group 1) to form salts
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Group 18: Noble Gases
•
•
•
•
•
Nonmetals
8 electrons in OEL (except helium which has 2)
Complete set of electrons in OEL
Unreactive
Colorless, odorless gases at RT
I can describe how chemical properties of elements are similar in the same
group.
I can label each group by name (ex: alkali metals, halogens, noble gases, etc.)
I can identify similar properties for each group.
I can explain which groups are likely to react together
Hydrogen
•
•
•
•
•
•
1 electron in OEL
Reactive
Colorless, odorless gas
Low density
Explosive reactions with oxygen
Most abundant element in the universe