ICP Unit 2

1
ICP Unit 2

• Fundamentals of Chemistry
• Chapters 17 and 19

2
First

• Go over tests
• Pass back homework
• New unit guide
• New style

3
Structure of the Atom
4
Parts of an Atom

• What are they?
• Where are they?
• What are their relative charges?
• What are their relative masses?
• What are protons, neutrons, and electrons made
  of?

5
Parts of an Atom
6
Elements

• What is an element?
• What do you know about symbols?

7
Some symbols based on old names

• What are some?
• Iron Fe
• Mercury Hg
• Potassium - K
• Sodium Na
• Silver Ag
• Gold Au
• Tin Sn
• Lead - Pb

8
How do we study such small things?

• What sort of things do scientists use to study
  small matter?
• Why are models useful?
• What are some examples of models?

9
Models of the atom

• Who were the first ones to think of matter as
  made up of atoms?
• What are some of the atomic models?

10
Atomic Models
1808
1897
1911
1913
11
Electrons

• Where are they?
• How do they travel?
• What is an electron cloud?

12
Fundamental Particles

• These are the most basic particles. Are atoms
  fundamental particles?
• Are protons, neutron, and electrons fundamental
  particles?
• Why not?

13
Quarks

• How many types are they?
• What are they a part of?
• Are they fundamental particles?

14
Atomic Masses

• Where is most of the mass of an atom?
• What units do we use for atomic masses?
• Why is that?

15
Atomic Masses

• Very tiny
• 1 amu 1.67 x 10-24 g
• What are the masses of a proton and a neutron?
• Electrons are 1,836 times smaller than protons
  and 1,837 times smaller than a neutron

16
Atomic Masses

• Where are they found?
• How are they calculated?
• Why dont we count electrons?
• Why arent atomic masses whole numbers on the
  periodic table?

17
Atomic Masses

• Molar mass/atomic mass shown on the periodic
  table is an average of the different masses for
  each element.
• What is the difference between the atomic mass
  and the molar mass?

18
Atomic Mass Summary

• Average of all masses of an element
• Found by adding protons and neutrons
• Units of atomic mass units (amu)
• Molar mass the same number, but in units of g/mol

19
How to Use the Periodic Table
20
Where is the Periodic Table?

• Found in the back cover of your book
• Or on the wall
• Or on R15 of your planner

21
How to Use the Periodic Table
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How to Use the Periodic Table
The symbol gives 1-2 letters to shorten the name
of the element.
23
How to Use the Periodic Table
The full name of the element is usually given at
the bottom.
24
How to Use the Periodic Table
The atomic number is the number of protons. This
is unique for each element.
25
How to Use the Periodic Table
The atomic mass is the sum of the protons and
neutrons in the average atom of the element.
26
Game

• Pick a partner and sit together
• You can use your book and planner, just not other
  teams papers
• If you dont have a calculator get one from the
  bench
• The team with the highest ratio of right/time
  gets an ECP

27
Game

• Go over answers

28
Neutral atoms

• Neutral atoms have no charge, which means the
  number of electrons the number of protons.
• How do we know how many electrons a neutral atom
  has?

29
Atoms

• The atomic mass is an average mass of an element.
  What do we call the atoms with different masses?

30
Isotopes

• How are different isotopes of the same atom
  similar?
• How are they different?

31
Practice

• Hydrogen has an average atomic mass of 1 and an
  atomic number of 1. How many neutrons are in the
  average atom of hydrogen?
• Cobalt has an average atomic mass of 59 and an
  atomic number of 27. How many neutrons are in the
  average atom of cobalt?

32
Advanced Practice

• An element has 12 neutrons and 13 protons. What
  is the element and what is its mass?
• An element has a mass of 235 amu and 143
  neutrons. What is the element?

33
Naming Isotopes

• How are they named?
• Can be written by the name followed by mass, or
  symbol with the mass in the upper left.
• Hydrogen-2 or 2H

34
Practice

• Write the symbols for the following
• Protons 3 Neutrons 5
• Protons 7 Neutrons 7
• Protons 108 Neutrons 170
• Mass 195 Neutrons 112
• Mass 19 Neutrons 5
• Mass 78 Neutrons 37

8Li 14N 278Hs 195Bi 19Si 78Nb
35
Atomic Mass

• What is it again?
• It is a weighted average, which means that it is
  the percentage x the mass of each isotope which
  are added together for the total average.

36
Carbon

• 98.93 Carbon-12
• 1.07 Carbon-13
• (98.9312 1.0713)/100 12.0107

37
Oxygen

• 99.757 Oxygen-16
• 0.038 Oxygen-17
• 0.205 Oxygen-18
• Determine atomic mass for Oxygen
• (99.757160.038170.20518)/100
• 16.004 amu

38
Isotopes Summary

• Isotopes are atoms of an element with varied
  numbers of neutrons
• Weighted average of masses is the average atomic
  mass
• Average atomic mass is what is shown on the
  periodic table

39
Project

• In groups of 2 draw Carbon-12 and Carbon-13 with
  the correct numbers of protons, neutrons, and
  electrons.
• Label the following
• Nucleus, protons, neutrons, electrons, electron
  cloud, Carbon-12, Carbon-13
• At the bottom explain the difference between them
  in 1-2 sentences.

40
Are they right?

• Are there any variations in figures?

41
The Periodic Table

• Who made the modern Periodic Table of the
  Elements?
• Periodic means repeating in a pattern. Does this
  make sense?
• How did he arrange it?

42
Famous Dead Guys

• Dmitri Mendeleev
• Russian 1834-1907
• Arranged the 63 known elements by mass on a
  periodic table and in groups by properties

43
Mendeleev

• Based on properties of the groups he could
  predict the masses and properties of undiscovered
  elements
• Arranged in order of mass, and noticed a pattern.

44
The Periodic Table

• What are the two sets (1 vertical and 1
  horizontal) of elements called?
• Which have similar properties?
• How many elements are there?

45
The Periodic Table
46
Group 1

• Alkali Metals
• What are some properties?
• Malleable, ductile, good conductors, very soft
  metals, very reactive, explosive in water, cesium
  and francium are some of the most reactive
  elements

47
Group 2

• Alkaline Earth Metals
• What are some properties
• Malleable, ductile, good conductors, very
  reactive, but less than alkali metals, never
  found free in nature

48
Groups 3-12

• Transition Metals
• Central block of metals
• What are some properties?
• Malleable, ductile, good conductors, some can
  produce magnetic fields, have unusual electron
  shells

49
Group 13-15 Metals

• Very dense solids
• Only 7
• What are they?
• Aluminum, Gallium, Indium, Tin, Thallium, Lead,
  and Bismuth

50
Group 13-16 Metalloids

• Found on the line between metals and nonmetals
• What is a metalloid?
• What are the 7 metalloids?
• Boron, Silicon, Germanium, Arsenic, Antimony,
  Tellurium, Polonium

51
Group 17

• Halogens
• Only group to have solids, liquids, and gases
• What are some properties?
• Nonmetals, insulators, form salts

52
Group 18

• Noble Gases
• Inert (dont react)
• The most stable elements

53
Lanthanides and Actinides

• 2 periods at the bottom of the chart
• Also called Rare Earth Metals
• Most are synthetic
• Most are radioactive
• Very heavy and unstable

54
Energy Levels

• Energy levels are set orbits at increasing
  distances from the nucleus

55
Electron Cloud

• Why might the number of electrons increase in
  each energy level?

56
Chapter 17 Review

• How are the elements arranged in the periodic
  table?
• What do the elements in a vertical (up and down)
  column of the periodic table have in common?
• How is an element defined?
• How is the atomic mass found?

57
1.

• The elements are arranged by increasing atomic
  number and by changes in physical and chemical
  properties.

58
2.

• The vertical columns in the periodic table are
  called groups elements in the same group have
  similar properties, such as electrical
  conductivity.

59
3.

• By the number of protons, this is unique to each
  element.

60
4.

• By adding the number of protons and neutrons in
  the nucleus. The protons can be found by looking
  at the periodic table because the number of
  protons is always equal to the atomic number.

61
Group Project

• Get in pairs and read the article on page 528
• Make a few notes on key points in the story
• Then read over the study guide on page 529

62
Group Project

• How are global average temperatures through time
  found?
• What other gases might be tracked by checking the
  ice records?
• What questions do you have on anything from
  Chapter 17?

63
Metals

• What are the properties of metals?
• What is luster?
• What does malleable mean?
• What does ductile mean?

64
Metals Bonding

• What is bonding?
• Why do they bond?
• Metals form ionic bonds.

65
Ions

• Charged atoms
• Caused by adding or removing electrons
• Cation positive ion
• Lost electron(s)
• Anion negative ion
• Gained electron(s)

66
Ions

• Atoms gain or lose electrons to be more like
  noble gases
• Charge equal to number of electrons gained or
  lost
• What is the charge on an electron?
• If something has a charge of 0 and loses an
  electron, what will the charge on the ion be?

67
Ionic Bonding

• One atom steals the electrons of another
• Metals have extra electrons they want to get rid
  of, nonmetals need electrons
• Nonmetals will steal the electrons from the
  metals, they both become more stable then

68
Ionic Bonding
69
Metallic Bonding

• What is it?
• Lots of cations (metals that have lost electrons)
  all have electrons flying around between them
• These spaces make them good conductors

70
Metallic Bonding
71
Alkali Metals

• What group are they?
• What are some properties?
• Will they become cations or anions?

72
Alkaline Earth Metals

• What group are they?
• What are some properties?
• Will they become cations or anions?

73
Transition Metals

• What groups are they?
• What are some properties?
• Will they become cations or anions?

74
Project

• Color in the blank periodic table based on
  Alkali, Alkaline Earth, and Transition Metals
• Give a key at the bottom listing properties of
  each group of metals
• Hold on to these, well use them again

75
Uses of Metals

• What group is used in fireworks?
• What metal is in marble?
• What does calcium do in your body?
• What 2 are used in medical procedures?
• What 3 are common in coins?
• Which is magnetic?
• Which are used in steel?

76
Ores

• What are they?
• Metals combined with other elements, found in the
  ground
• Separated by crushing the rock and separating the
  compounds and elements

77
Mining
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Lanthanides and Actinides

• What is the other name for them?
• What are the elements 58-71?
• What are the elements 90-103?
• Why are they listed below the periodic table?

79
Lanthanides

• Why are they called the Lanthanides?
• All but 1 are naturally occurring, Promethium is
  man-made

80
Actinides

• Why are they called the Actinides?
• Only 3 are naturally occurring, Thorium,
  Protactinium, and Uranium
• What is special about Uranium?
• What property do all Actinides share?

81
Nonmetals
82
Nonmetals

• What are some properties?
• Where are they?
• Parts of Groups 14-16 and all of 17 and 18.

83
Nonmetals Bonding

• How do metals bond?
• How do nonmetals bond?
• What is covalent bonding?

84
Covalent Bonding

• Sharing electrons
• Bonding between nonmetals, usually

85
Nonmetal Bonding
86
Bonding Practice

• Would these be metallic, ionic, or covalent
• Na and Cl
• Au and Ag
• Cs and S
• P and O
• I and Zr
• C and O
• Mg and O

87
Hydrogen

• Where is it on the periodic table?
• Is it a metal, nonmetal, or metalloid?
• Extremely reactive element, combines easily with
  oxygen as combustion

88
Combustion of Hydrogen
89
Hydrogen

• How common is it in the universe?
• Most on Earth is in water
• Hydrogen as an element is diatomic, what does
  this mean?

90
Diatomic Elements

• There are 7 elements that are naturally found as
  diatomics
• This means they are most stable bonded in pairs
• H2, N2, O2, F2, Cl2, I2, Br2

91
Halogens

• Which group are they?
• What is formed when they bond with metals?
• What is the most reactive halogen?

92
Halogens
93
Hydrogen

• Hydrogen can fit in a couple different places on
  the periodic table. Get in groups of 4 and
  discuss in which place it fits best, then write a
  few sentences summarizing your argument. We will
  discuss it shortly.

94
Hydrogen

• Argue for hydrogen belonging in Group 1
• Argue for hydrogen belonging in Group 17

95
Noble Gases

• Dont combine with other elements naturally
• What makes them so stable?

96
Project

• Fill in the nonmetals and noble gases on your
  periodic table

97
Sublimation

• Think back to phase (states of matter) changes.
  What are they?
• Gas ? Liquid
• Liquid ? Gas
• Liquid ? Solid
• Solid ? Liquid
• Solid ? Gas

98
Sublimation

• Solids becoming a gas, skipping liquid phase
• Very few elements sublime, takes a lot of energy

99
Metalloids

• Boron, Silicon, Germanium, Arsenic, Antimony,
  Tellurium, Polonium
• What are they used in?

100
Carbon

• Where do you find carbon?
• What are some different compounds made only of
  carbon?
• These are called allotropes

101
Potatoes

• When theyre in the ground theyre potatoes
• When theyre smashed and heated theyre mashed
  potatoes
• When theyre combined with milk and boiled
  theyre called potato soup
• When theyre fried theyre potato chips
• All are different ways of using the same thing,
  but theyre all a potato
• This is what an allotrope is

102
Carbon

• Graphite, diamond, and Buckminsterfullerene are
  all compounds containing only carbon

103
Oxygen

• 2 main ways oxygen is found in the air, what are
  they?
• O2 we breathe this, all large life depends on
  it
• O3 the ozone layer limits radiation

104
Synthetic Elements

• Synthetic means they arent found in nature,
  theyre man-made
• How are they made?

105
Transuranium Elements

• What does this mean?
• All have more than 92 protons, very heavy and
  unstable
• Some of the more stable ones have uses, such as
  plutonium and americium

106
Project

• Finish your periodic table
• When youre done bring it up and trade for a
  review packet
• You will get the table back before the test

107
End of Unit

• Any Questions?