1. Chapter 17 Properties of Atoms and the Periodic Table Section 3
Page 516-

2. Atomic Models Ancient Greek- “cannot be divided”
John Dalton’s Theory- simple sphere
Thompson’s Model- plum pudding
Rutherford- Electron/Proton Model
Bohr- Orbital Model/ Neutron
Modern – electron Cloud Model
Protons charge, 1amu
Neutrons 0 charge, 1amu
Electrons charge, negligible mass

3. Review- Section 1
Elements are abbreviated in scientific shorthand- first letter or 2 letters of element name.
Atom- smallest piece of matter that still has the properties of the element.
Protons have electrical charge of 1+
Neutrons do not have an electrical charge
Electrons have electrical charge 1-
Protons and neutrons are made up of smaller particles called quarks. Page
Six quarks are known to exist; the sixth is called the top quark.
Scientists use scaled-up models to represent atoms.
Early models of atoms used a solid sphere
Current models show electrons traveling in specific energy levels around a nucleus of protons and neutrons.

4. Review Section 2
Mass of the atom composed mostly of the protons and neutrons in the nucleus.
Unit of measurement of mass for atomic particles is atomic mass unit (amu) which is one twelfth the mass of a carbon atom containing 6 protons and 6 neutrons.
Atomic number (Z)the number of protons in an atom; number of protons identifies the element.
The sum of the number of protons and neutrons in the nucleus of an atom is the mass number (atomic mass) (A)
Isotopes- atoms of the same element with different numbers of neutrons.
Different isotopes have different nuclear properties.
Number of neutrons is equal to the mass number minus atomic number.

5. Identifying Numbers (P512)
The atoms of each elements contain a unique numbers of protons.
The atomic number of an element is the number of protons in the nucleus of an atom of that element. (Z)
Atoms of an element are identified by the number of protons because this number never changes without changing the identify of the element. The number of electrons equals the number of protons so charge is neutral

6. Number of Neutrons
Most atoms of carbon have six neutrons, some have 7 and some have 8.
They are all carbon atoms because they all have six protons. (6 electrons)
These three kinds of carbon atoms are called isotopes. Isotopes (I suh tohps) are atoms of the same element that have different numbers of neutrons. (P514)

7. Atomic Mass Number
The mass number of an isotope is the number of neutrons plus protons. Also called the atomic mass number. (A)

8. Atomic Number, Atomic Mass, and # of Neutrons
mass number = #protons + # neutrons
atomic number = # protons
Number of neutrons = mass number – atomic number
Number of neutrons = A – Z

9. Symbols for the Elements
The symbols for the elements are either one- or two- letter abbreviations, often based on the element name.
For example, V is the symbol for vanadium, and Sc is the symbol for scandium.
Sometimes the symbols don’t match the names.
In those cases, the symbol might come from Greek or Latin or German names for the elements.

10. Isotope Identification Name of element followed by mass number identifies the isotope.
Hyphen notation
Carbon or C-14
Mass number
Atomic number
14 6 C C

11. Average Atomic Mass
Weighted average of the atomic masses of all the isotopes.
Weighted on the relative abundance of the isotopes.
Periodic table gives average atomic mass
Average atomic mass is closest to the element’s most abundant isotope.

12. Find the number How many neutrons in Iodine-131?
What is the atomic mass number of a copper isotope with 34 neutrons?
Worksheet

13. Development of the Periodic Table– Mendeleev’s Table of Elements
A Russian chemist, Dmitri Mendeleev (men duh LAY uhf), published his first version of the periodic table 1869.
When Mendeleev arranged the elements in order of increasing atomic mass, he saw a pattern.
He noticed repeating patterns of properties.

14. Development of the Periodic Table– Mendeleev’s Table of Elements
To make his table work, Mendeleev had to leave three gaps for missing elements.
Based on the groupings in his table, he predicted the properties for the missing elements.
Within 15 years, all three elements—gallium, scandium, and germanium—were discovered.
The most important characteristic of a good scientific theory is the ability to predict future discoveries.

15. Moseley’s Contribution
Although Mendeleev’s table correctly organized most of the elements, a few elements (cobalt and nickel, tellurium and iodine) seemed out of place.
In the early twentieth century, the English physicist Henry Moseley realized that Mendeleev’s table could be improved by arranging the elements according to atomic number rather than atomic mass.

16. Today’s Periodic Table

17. Today’s Periodic Table
In the modern periodic table, the elements still are organized by increasing atomic number.
The rows or periods are labeled 1-7.
A period is a row of elements in the periodic table whose properties change gradually and predictably.

18. Today’s Periodic Table
The periodic table has 18 columns of elements.
Each column contains a group, or family, of elements.
A group contains elements that have similar physical or chemical properties.

19. Element Key Color- book only not reference sheet Blue – Metal
Green – Metalloid
Yellow - Nonmetal

20. Common elements - Uncommon Names
Sodium Na Natrium
Potassium K Kalium
Iron Fe Ferrum
Copper Cu Cuprum
Silver Ag Argentum
Tin Sn Stannum
Antimony Sb Stibium
Tungsten W Wolfram
Gold Au Aurum
Mercury Hg Hydragyrum
Lead Pb Plumbum

21. Zones on the Periodic Table
The periodic table can be divided into sections.
One section consists of the first two groups, Groups 1 and 2, and the elements in Groups These are the main group elements or Representative Elements

22. Zones on the Periodic Table
Main Groups
The main group elements include metals, metalloids, and nonmetals. They are sometimes called representative elements.

23. Zones on the Periodic Table
The elements in Groups 3-12 are transition elements. They are all metals so they are sometimes called the transition metals.

24. Zones on the Periodic Table
Some transition elements, called the inner transition elements, are placed below the main table. These elements are called
the lanthanide and actinide series because one series follows the element lanthanum, element 57, and the other series follows actinium, element 89.

25. Electron Configuration
Electrons within the electron cloud have different energy levels.
Each electron is assigned 4 different “quantum numbers”. No two electrons within an atom can have the same quantum numbers.
Energy Level quantum number, there are 7 levels (1-7)
Shape quantum number -suborbits for electrons s,p,d,f
Orientation quantum number
Spin quantum number- right handed or left handed

26. Electron Energy Levels
Lowest energy near the nucleus
Highest energy far from the nucleus
Energy Levels Overlap
Shapes- s,p,d,f
s- 2 electrons
p- 6 electrons
d- 10 electrons
f- 14 electrons
Spin - right or left

27. Review Periodic Table
Mendeleev- arranged in order of increasing atomic mass.
Moseley – in order of increasing atomic number
Atomic mass = #protons + # neutrons, atomic number = #protons
Period- row of elements, properties change gradually
Group – column of elements, similar properties
Element key – name, symbol, atomic number, average atomic mass
Zones- main group elements, transition metals
Electron configuration – all the elements in a group have the same configuration of electrons in their outer shell

28. Energy Levels and Shapes18
1s2 2
2s2
2p6 8
3s2
3p6 8
5s2
4d10
5p6 18
6s2
5d10
6p6
4f14 32
7s2
6d10
7p6
5f14 32

29. Electrons and Periods
Each period of the periodic table represents a different energy level and a different number of total electrons.
Period 1 - Energy Level 1 – up to 2 electrons 2 elements
Period 2 – Energy Level 2- up to 8 electrons elements
Period 3- energy Level 3 – up to 8 electrons elements
Period 4 - energy Level 4 - up to 18 electrons including 10 from level elements
Period 5 - Energy Level 5 up to 18 electrons including 10 from level elements
Period 6 - Energy Level 6 up to 32 electrons including 14 from level Elements
Period 7 - Energy Level 7 up to 32 electrons including 14 from level elements

30. Electrons in groups Group 1 – 1 electron in outer shell s1
Group 2 – 2 electrons in outer shell s2
Group 3-12 many electrons in outer shell
Group electrons in outer shell
Group 14 – 4 electrons in outer shell
Group 15 – 5 electrons in outer shell
Group electrons in outer shell
Group 17 – 7 electrons in outer shell
Group electrons in outer shell

31. Electron Dot Diagrams
Page 522 H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Kr Rb Sr Xe Cs Ba Rn Fr Ra

32. Review Electron Configuration
The properties of an element are determined by the arrangement of electrons in the outer energy level.
The number of electrons in the outer energy level of main group elements can be determined by the group number of the element.
Group 1 and 2: number of electrons = group number.
Group 13-18: number of electrons = group number - 10

33. Liquids and Synthetics
Two elements on the periodic table are liquids at room temperature.
Their logo is a drop. What are they?
Elements that do not occur naturally on Earth are marked with a bull’s-eye logo.
These are synthetic elements.

34. Gases
All the gases except hydrogen are on the right side of the table.
They are marked with a balloon logo.
Most of the other elements are solids at room temperature and are marked with a cube.

35. Diatomic Gases Br2- bromine I2 – iodine N2 – nitrogen Cl2 - chlorine
H2 – hydrogen
O2 – oxygen
F2 – fluorine
Mr. BrINClHOF

36. Synthetic Elements Newly synthesized elements are given a
temporary name and 3-letter symbol that is related to the element’s atomic number.
Once the discovery of the element is verified, the discoverers can choose a permanent name.

37. In the beginning
When God started building the atoms of elements he began with a design. We may have discovered that design.
He began adding electrons, protons and neutrons according to the design.
The first element had 1 electron and 1 proton and either 0,1 or 2 neutrons.
The second element had 2 electrons and 2 protons and either 1,2 or 3 neutrons.

38. Elements and Their Properties Chapter 19, page 570
Metals
Group 1
Group 2
Group 13-17
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Group 18 – Noble Gases

39. Metals, Non-metals, Metalloids P570
If you look at the periodic table, you will notice it is color coded.
Blue- metals
Yellow-non metals
Green-metaloids

40. Metals P570
With the exception of mercury, all the metals are solids, most with high melting points.
A metal is an element that has luster, is a good conductor of heat and electricity, is malleable, and is ductile.
The ability to reflect light is a property of metals called luster.

41. Nonmetals
Nonmetals are usually gases or brittle solids at room temperature and poor conductors of heat and electricity.
There are only 17 nonmetals, but they include many elements that are essential for life—carbon, sulfur, nitrogen, oxygen, phosphorus, and iodine.

42. Metalloids
The elements between metals and nonmetals on the periodic table are called metalloids.
A metalloid is an element that shares some properties with metals and some with nonmetals.
Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium, Polonium, Astatine

43. Groups 1 and 2
Groups 1 and 2 are always found in nature combined with other elements.
They’re called active metals because of their readiness to form new substances with other elements.
They are all metals except hydrogen, the first element in Group 1.
Although hydrogen is placed in Group 1, it shares properties with the elements in Group 1 and Group 17.
Group 1 atoms have 1 electron in the outer most suborbits. s1
Group 2 atoms have 2 electrons in the outer most suborbits. s2

44. Group 1 Alkali Metals
The Group 1 elements have a specific family name—alkali metals.
low densities and low melting points.
All the alkali metals are silvery solids with
These elements increase in their reactivity, or tendency to combine with other substances, as you move from top to bottom.

45. Group 2 Alkaline Earth Metals
Next to the alkali metals are the alkaline earth metals.
and has a higher melting point than the alkali metal in the same period.
Each alkaline earth metal is denser and harder
Alkaline earth metals are reactive, but not as reactive as the alkali metal in the same period.

46. Groups 13 through 18
The elements in Groups are not all solid metals like the elements of Groups 1 and 2. In
fact, a single group can contain metals, nonmetals, and metalloids and have members that are solids, liquids, and gases.

47. Group 17—The Halogen Group
All the elements in Group 17 are nonmetals except for astatine, which is a radioactive metalloid.
These elements are called halogens, which means “salt-former.”
All of the halogens form salts with sodium and the other alkali metals.
The most reactive halogens is fluorine and reactivity decreases as we move down to chlorine, bromine, iodine.

48. Group 18—The Noble Gases
The Group18 elements are called the noble gases.
This is because they rarely combine with other elements and are found in nature only as uncombined elements.
Their reactivity is very low. They are too noble to associate with other elements

49. Group 18—The Noble Gases
Helium is less dense than air, so it’s great for all kinds of balloons.
Even though hydrogen is lighter than helium, helium is preferred because it will not burn (because it is noble).
Helium balloons lift instruments into the upper atmosphere to measure atmospheric conditions.

50. Uses for the Noble Gases
The “neon” lights you see in advertising signs can contain any of the noble gases, not just neon.
Electricity passing through the glass tubes make the gas glow. Each noble gas glows a different color.
Helium glows yellow, neon glows red-orange, and argon produces a bluish-violet color.

51. Uses for the Noble Gases
At the bottom of the group is radon, a radioactive gas produced naturally as uranium decays in rocks and soil.
If radon seeps into a home, the gas can be harmful because it continues to emit radiation.
When people breathe the gas over a period of time, it can cause lung cancer.
To sell your house you must check for radon gas.

52. Group 13—The Boron Family
The elements in Group 13 are all metals except boron, which is a brittle, black metalloid.
Aluminum is used to make soft-drink cans, cookware, siding for homes, and baseball bats.
Gallium is a solid metal, but its melting point is so low that it will melt in your hand.
It is used to make computer chips.

53. Group 14—The Carbon Group
The nonmetal carbon exists as an element in several forms.
You’re familiar with two of them—diamond and graphite.
Allotropes- different forms of the same element having different molecular structure.
Carbon is the basis of all living things.

54. Group 14—The Carbon Group Silicon
Carbon is followed by the metalloid silicon, an abundant element contained in sand.
Sand contains ground up particles of minerals such as quartz, which is composed of silicon and oxygen.
Glass is an important product made from sand.

55. Group 14—The Carbon Group
Silicon and its Group 14 neighbor, germanium, are metalloids.
They are used in electronics as semiconductors.
A semiconductor conducts electricity under some conditions but not others.
Sand contains ground up particles of minerals such as quartz, which is composed of silicon and oxygen.

56. Group 14—The Carbon Group
Tin and lead are the two heaviest elements in Group 14.
Lead is used to protect you during dental X rays, protective shielding around nuclear reactors, and containers used for storing and transporting radioactive materials.
Lead was once used in paints but because it is toxic, lead is no longer widely used.
Lead also is used in car batteries- caution
Tin is used in pewter, toothpaste, and the coating on steel cans used for food.

57. Group 15—The Nitrogen Group
Nitrogen and phosphorus are required by living things and are used to manufacture various items.
These elements also are parts of the biological materials that store genetic information and energy in living organisms.

58. Group 15—The Nitrogen Group
Although almost 80 percent of the air you breathe is nitrogen, plants and animals can’t get the nitrogen needed by breathing nitrogen gas.
Bacteria in the soil must first change nitrogen gas into substances that can be absorbed through the roots of plants.
Then, by eating some plants, nitrogen becomes available to your body.

59. Group 15—The Nitrogen Group
The element phosphorus comes in two forms—white and red.
White phosphorus is so active it can’t be exposed to oxygen in the air or it will burst into flames.
The heads of matches contain the less active red phosphorus, which ignites from the heat produced by friction when the match is struck.

60. Group 15—The Nitrogen Group
Phosphorous compounds are essential ingredients for healthy teeth and bones.
Plants also need phosphorus, so it is one of the nutrients in most fertilizers.

61. Group 16—The Oxygen Family
The first two members of Group 16, oxygen and sulfur, are essential for life.
The heavier members of the group, tellurium and polonium, are both metalloids.

62. Group 16—The Oxygen Family
About 20 percent of Earth’s atmosphere is the oxygen you breathe.
Oxygen is abundant in Earth’s rocks and minerals because it readily combines with other elements.
Oxygen also is required for combustion to occur.

63. Group 16—The Oxygen Family sulfur
Sulfur is a solid, yellow nonmetal.
Large amounts of sulfur are used to manufacture sulfuric acid, one of the most commonly used chemicals in the world.
Sulfuric acid is a combination of sulfur, hydrogen, and oxygen.
It is used in the manufacture of paints, fertilizers, detergents, synthetic fibers, and rubber.

64. Group 16—The Oxygen Family
Selenium conducts electricity when exposed to light, so it is used in solar cells, light meters and photographic materials.
Its most important use is as the light-sensitive component in photocopy machines.
Traces of selenium are also necessary for good health.

65. Why do elements behave as they do?
To explain why, scientist developed a theory.
Elements behave as they do (react or combine with other elements) because of the position of the electrons.
The electrons in the outer orbits (highest energy level) determine the chemical properties of an element.
8 electrons in the outer orbits is a “magic” number (full outer orbit)

66. The “magic” 8
For elements with atomic number >2, the magic number is 8 electrons in the outer orbits.
s2p6
The Noble gases have 8 electrons
Elements with fewer electrons combine with other elements in ways that produce 8 electrons in the outer orbits.
Elements with few electrons lose electrons to “make 8”.
Elements with many electrons gain electrons to “make 8”.

67. Outer electrons by Group
Tendency
Group 1- Hydrogen, Lithium 1
Lose 1
Group 2 Beryllium 2
Lose 2
Group 13 Boron 3
Lose 3
Group 14 Carbon 4
Lose 4 or gain 4
Group 15 Nitrogen 5
Gain 3
Group 16 Oxygen 6
Gain 2
Group 17 Fluorine 7
Gain 1
Group 18 Helium, Neon 8
Happy as a clam

68. The Metals in the Middle
Groups 3-12 are called the transition elements.
All of them are metals, so they are sometimes called transition metals.
Across any period from Group 3 through 12, the properties of the elements change less noticeably than they do across a period of representative elements.
Most transition elements are found combined with other elements in ores.

69. The Iron Triad
Three elements in period 4—iron, cobalt, and nickel—have such similar properties that they
are known as the iron triad.
These elements, among others, have magnetic properties.

70. The Iron Triad
Industrial magnets are made from an alloy of nickel, cobalt, and aluminum.
Nickel is used in batteries along with cadmium.
Iron is a necessary part of hemoglobin, the substance that transports oxygen in the blood.
Iron also is mixed with other metals and with carbon to create a variety of steels with different properties.

71. Uses of Transition Elements
Most transition metals have higher melting points than the main group elements.
The filaments of lightbulbs are made of
tungsten, element 74.
Tungsten has the highest melting point of any metal (3,410°C) and will not melt when a current passes through it.

72. Chapter 17 Assignments Note Taking Worksheet Atomic Mass worksheet
Periodic Table worksheet
Chapter Review Page 530:1-18, 27
Monday- Complete Periodic Table
Tuesday – Writing Test
Wednesday – Chapter Review
Thursday- Friday
Chapter 19 Elements and their properties
Monday – Chapter 19 Note Taking Worksheet
Tuesday - Test

73. Uses of Transition Elements
Mercury, which has the lowest melting point of any metal (–39°C), was used in thermometers and in barometers.
Mercury is the only metal that is a liquid at room temperatures.
Like many of the heavy metals, mercury is poisonous to living beings.

74. Catalytic Converter
The catalytic converter on a car uses platinum, palladium, and rhodium as catalysts to speed up a chemical reaction that removes toxic fumes from the exhaust of the car.
The catalytic converter contains about $200 worth of these metals which can be sold on the black market.

75. Precious (coinage) Metals
Copper, Silver, Gold, Platinum
Metal Properties
Malleable and Ductile
Can be shaped into beautiful objects
Rare
Valuable
Often used for coins

76. Element Practice Element: Iron Symbol _________ Period ________
Group ________
Atomic Number __________
Average Atomic Mass __________

77. Element Practice Element: Oxygen Symbol ________ Period ________
Group ________
Atomic Number __________
Average Atomic Mass __________

78. Element Practice Element: Sodium Symbol _______ Period ________
Group ________
Atomic Number __________
Average Atomic Mass __________

79. Element Practice Element: Neon Symbol _______ Period ________
Group ________
Atomic Number __________
Average Atomic Mass __________

80. Element Practice Element: Tungsten Symbol _______ Period ________
Group ________
Atomic Number __________
Average Atomic Mass __________

81. Element Practice Element: Iodine Symbol _______ Period ________
Group ________
Atomic Number __________
Average Atomic Mass __________