Particles of Matter

1

• Particles of Matter
• Page 10, 11 and 12 of binder

2

• To understand what makes one type of matter
  different from another requires an understanding
  of ATOMS. The concept of the atom has been around
  a long time. A major question among Greek
  philosophers involved the divisibility of matter.
  A stone broken into fragments or even ground into
  a powder was still stone.
• Could the subdivision of matter continue
  forever, or was there a smallest unit of matter?

3
Ancient Atomic TheoryAristotle- Greek
PhilosopherMatter is made of Earth, Air, Fire,
WaterDemocritus- GreekMatter is made up of
small particles called atoms
4
John Dalton 1802, an English schoolteacher,
proposed a new atomic theory
5
Daltons Particle Theory
6

• Daltons Atomic Theory
• 1. Atoms are the smallest form of matter.
• 2. In any element, all the atoms are exactly
  alike.
• (protons (), Electrons (-) and neutrons)
• 3. Atoms of two or more elements can combine to
  form compounds.
• 4. The elements in a compound are always in a
  constant ratio. For example, water is a compound
  made of oxygen atoms and hydrogen atoms. If you
  compare any sample of pure water to any other
  sample of pure water, the ratio of hydrogen(2) to
  oxygen(1) is always the same.

7

• Once Dalton's atomic theory was accepted,
  scientists began trying to prove the existence of
  the atom and gain an understanding of its
  structure. Like an onion being peeled, atomic
  structure was revealed from the outside in.
• The first subatomic particle discovered was the
  ELECTRON. Electrons are tiny, negatively charged
  particles that move around the center of an atom
  in what are called electron clouds. It is the
  edge of the electron cloud which signifies the
  outer edge of the atom.
• The center is called the NUCLEUS (Latin for
  "little nut"). Over 99.9 of the mass of an atom
  is in the nucleus, yet the nucleus accounts for
  less than .01 of atomic length. Thus, an atom
  and everything made up of atoms is mostly empty
  space.

8

• Inside the nucleus are the PROTON and the
  NEUTRON. As their names imply, neutrons are
  neutral (have no electrical charge), whereas
  protons have a positive charge. Because atoms are
  by definition neutral particles, the number of
  protons in an atom equals the number of
  electrons.

Now You KnowIf the nucleus of an atom were the size of a tennis ball, the entire atom would be about six miles in diameter.
9
Atomic StructureThe Bohr Model
10
While there are millions of different types of
materials, there is an order and structure to
explain how elements are combined. These hundred
elements combine to form billions of materials.
This compares to the way the 26 letters in our
alphabet combine to form millions of words.

• How is Matter Constructed?
• From the smallest particles to larger
  combinations of particles
• Building Matter
• Sub Atomic Particles (Electrons, Protons,
  Neutrons) ---gt Atoms ---gt Molecules-- gtElements
  ----gt Compounds

11
Current Atomic Structure

• Atomic Particles
• Protons () Electrons (-) and Neutrons (neutral)
• B. Because atoms are neutral particles, the
• number of protons () the number of electrons
  (-)
• C. Most of the atom is empty space
• D. Nucleus (Protons () and Neutrons)
• comprises 99.9 of an atom's mass.

12
Overview of the Periodic Table

• 3,2,1 Activity
• Three things you know about the Periodic Table
• Two things you would like to know about the
  Periodic Table.
• One thing you think is going to be challenging
  when studying the Periodic Table

13
Unit 3Elements and the Periodic Table

• Section 1 Organizing the Elements
• Pages 57 to 61

14
Mendeleev created a table organized by increasing
atomic mass. 
15
Modern Periodic Table organized by increasing
atomic number
16
I Current Atomic Structure

• Atomic Particles
• Protons () Electrons (-) and Neutrons (neutral)
• Most of the atom is
• empty space
• Nucleus comprises 99.9 of an atom's mass
• Atoms are electrically neutral when
• protons electrons

17
II Energy Levels

• Electrons orbit nucleus in energy levels called
  energy shells (orbitals)
• Each atom has seven energy shells (orbitals).
• Electrons in outer shell (orbitals) are
  unstable.
• A happy atom has 8 electrons in the outer shell
  (orbitals) and fulfills the Octet Rule.

18
The Electron Hotel
Shell Number (Hotel Floor) Electron Capacity (Hotel Rooms) Chlorine Atom Atomic Number 17
1 2
2 8
3 8
4 18
5 18
6 36
7 36
19
III Atomic Number

• Atomic Number protons in the atom
• Element 26 is Iron. Iron has 26 protons in its
  nucleus

20
Atomic Number
21
Modern Periodic Table organized by increasing
atomic number
22
IV Atomic Mass

• Atomic Mass
• protons of neutrons in nucleus
• Atomic Mass Unit 1/12 the mass of a carbon atom

23
Atomic Mass
24
(No Transcript)
25
Element Name Atomic Number of Protons of
Electrons Atomic Mass of Neutrons Electron
Configuration Family or Group Period
Magnesium
12
12
12
24
12
2 8 2
2
3
Element Name Atomic Number of Protons of
Electrons Atomic Mass of Neutrons Electron
Configuration Family or Group Period
Carbon
6
6
6
12
6
2 4
4
2
26
Element Name Atomic Number of Protons of
Electrons Atomic Mass of Neutrons Electron
Configuration Family or Group Period
Hydrogen
1
1
1
1
0
1
1
1
Element Name Atomic Number of Protons of
Electrons Atomic Mass of Neutrons Electron
Configuration Family or Group Period
Potassium
19
19
19
39
20
2 8 8 1
1
4
27
Isotopes
Fat Cousins

• An atom with varying number of neutrons but the
  number of protons stays the same.

28
Isotopes
29
Hydrogen (Normal) Deuterium (Isotope)
Tritium (Isotope)
1 proton 1 proton
1 proton 0 neutrons
1 neutron
2 neutron 1 electron
1 electron
1 electron
Isotopes of Hydrogen
30
Normal Carbon (Carbon 12) Carbon 13
Carbon 14 6 protons
6 protons
6 protons 6 neutrons
7 neutrons 8
neutrons 6 electrons 6
electrons 6 electrons
Isotopes of Carbon
31
Ions charged elements

• In a stable element, the p e and has a
  neutral charge.
• However, in an attempt to bond, an atom may lose
  or gain electrons from its outer most energy
  level in an attempt to fulfill the Octet Rule.
• If an element loses an electron, it obtains a
  positive charge because it has an extra proton
  in the nucleus.
• If an element gains an electron, it obtains a
  negative charge because of the extra electron.

32
Periodic Table

• Periods horizontal rows
• As you move from left to right in a horizontal
  row, the number of electrons in each atom
  increases by one electron.
• The final element in each row has eight
  electrons in its outer shell, which fulfills the
  Octet Rule.
• The last vertical column of elements are the
  very stable noble gases- very stable and
  nonreactive.

33
Periodic Table

• Families- i.e. Groups- vertical columns
• As you move down the column, the number of
  energy levels containing electrons increases by
  one.

34
Determining Valence Numbers i.e. Oxidation
Numbers

• Valence Number is the charge of an atom after it
  fulfills the Octet Rule
• of e- in outer shell 1 2 3 4
  5 6 7 8
• What atom does to
• fulfill Octet Rule
• Gain or Loss e- -1 -2
  -3 - 4 3 2
  1 0
• Valence Number 1 2 3
  -4 -3 -2 -1
  0
• Elements H
  He
• Li Be
  B C N O F
  Ne
• Na Mg Al Si P S
  Cl Ar
• K Ca

35
of e- in outer shell
1 2 3 4 5
6 7 8What atom does to fulfill
Octet Rule Gain or Loss e-
-1 -2
-3
- 4 3 2 1 0Valence Number
1 2

3 -4 -3 -2 -1 0
36
Element Name Atomic Number of Protons of
Electrons Atomic Mass of Neutrons Electron
Configuration Family or Group Period Gain or
Loss Electrons Valence or Oxidation
Nitrogen
7
7
7
14
7
2 5
5
2
Gain 3
-3
Element Name Atomic Number of Protons of
Electrons Atomic Mass of Neutrons Electron
Configuration Family or Group Period Gain or
Loss Electrons Valence or Oxidation
Calcium
20
20
20
40
20
2 8 8 2
2
4
Loss 2
2
37
Element Name Atomic Number of Protons of
Electrons Atomic Mass of Neutrons Electron
Configuration Family or Group Period Gain or
Loss Electrons Valence or Oxidation
Neon
10
10
10
20
10
2 8
8
2
Neither
0
38

• Standard Deviant Video Tape 1
• Balancing chemical equations
• Mass number
• Atomic number
• Isotopes
• Ions
• amus

39
IX Chemical Equations

• Valence Numbers Number of Oxygen
  atoms
• C 4 0 -2 C 4 O-2 O-2 CO2
  Carbon Dioxide
• Na1 Cl -1 NaCl Table Salt
• H 1 Cl -1 HCl Hydrochloric Acid
• Na 1 H 1 0 -2 NaOH Sodium
  Hydroxide

40
X Types of Bonding

• Ionic Bonding transfer of one or more electrons
  from one atom to another to fulfill the octet
  rule.
• Example
• Sodium Na (1) Chloride Cl (-1) NaCl
  Sodium Chloride
• Elements that lose electrons easily and form
  positive ions are called metals such as gold,
  silver, iron and copper.
• Elements that gain electrons easily and form
  negative ions are called nonmetals such as
  nitrogen, oxygen, chlorine and sulfur.

41
Ionic Bonds
42

• Standard Deviants Video Tape 2
• Chemical Bonding

43
Types of Bonding

• Covalent Bonding sharing of one or more
  electrons between two atoms.
• Example
• Carbon (-4) 4 Hydrogen (l) CH4 Methane

44
Covalent Bonds
45
Element Name Atomic Number of Protons of
Electrons Atomic Mass of Neutrons Electron
Configuration Family or Group Period Gain or
Loss Electrons Valence or Oxidation
Phosphorus
15
15
15
31
16
2 8 5
5
3
Gain 3
-3
Element Name Atomic Number of Protons of
Electrons Atomic Mass of Neutrons Electron
Configuration Family or Group Period Gain or
Loss Electrons Valence or Oxidation
Lithium
3
3
3
7
4
2 1
1
2
Loss 1
1
46
Sample Quiz

• Your assigned element is _________________________
  __
• 1. What is the atomic number of the element?
• 2. How many neutrons does the element have in
  its nucleus?
• 3. What is the family number for the element?
  
• 4. How many electrons does the element have in
  its outer shell?
• 5. Does the atom want gain or lose electron
  from its outer shell to fulfill the Octet Rule?
  
• 6. What is the valence number for element?
• 7. What is the period number for the element?
• 8. How many electron energy levels is the
  element using?
• 9. Is the element classified as a Metal,
  Nonmetal, or Noble gas?