1. Periodic Table of Elements
MEET THE ELEMENTS
Pages
Ch.4.1, 4.2, 4.3, 4.4 and 5.1

2. Dmitri Mendeleev
He recognized patterns in the element’s approximate atomic masses and their ability to bond with other elements.

3. Periodic Table
Based on atomic masses and their ability to bond with other elements, Mendeleev constructed the first periodic Table.

4. The Atom
Nucleus: The core of the atom that contains two different subatomic particles.

5. The Atom cont… Protons: Have a positive charge.
The number of protons equals the number of electrons.

6. Neutrons: Have no Charge.
The Atom cont…
Neutrons: Have no Charge.

7. Electrons Negative charge.
The Atom cont…
Electrons Negative charge. .

8. Atomic Numbers, Symbols and Mass
Atomic number is the smaller number and the number of protons in the nucleus.
Element Symbol 47 Ag
Silver
Element Name
Atomic mass is the average mass of all the known isotopes.

9. How to calculate # of neutrons
Mass number - Atomic number = # of neutrons
This element is Nitrogen. Its mass # is 14. So mass # of 14, minus atomic # of 7, equals 7 neutrons.
Count the number of protons. What element is it?

10. How to Calculate Number of Electrons
The number of electrons equal the number of protons.
7 electrons
7 protons

11. How many neutrons does Mn (Manganese) have?30 25 55 7 30

12. How many Neutrons does K (Potassium) have?19 20 39 11 10
0 of 30

13. How many Protons does Hg Have?30 80
200
120

14. How many Electrons does Hg Have?30 80
200
120

15. Isotopes
When atoms of the same element have a different number of neutrons

16. Valence Electrons
The electrons on the outermost ring or energy level that can be shared or transferred with other atoms to make compounds.

17. Valence Electrons and Bonding (ch. 5.1 pgs. 176-182)
The number of valence electrons in an atom of an element determines many properties of that element, including the ways in which the atom can bond with other atoms.

18. When an atom has a different # of neutrons it’s called a…
Ion
Isotope
Proton
Element
0 of 30

19. What subatomic particle influences an elements ability to bond?30
Protons
Neutrons
Valence Electrons
Nucleus

20. Groups –Families
elements
in a
group
have very
similar characteristics
i.e. bonding, reactivity, valence electrons
Periods- elements in a period are not alike, but gradually change as you move from left to right.

21. Almost 75% of all elements are classified as metals.

22. Properties of Metals
Conductors: Metals are good at conducting electricity.
Malleable: Ability to bend or pound into shapes.

23. Properties of Metals Ductile: Pull or stretch into wire.
Many are shiny, hard and magnetic.
High melting point

24. Which of the following would be the best conductor of electricity?
Carbon (atomic number 6)
Strontium (atomic number 38)
Tellurium (atomic number 52) of 30

25. What is a characteristic of metals?
Gas
Stable
Good conductor
Brittle 30

26. Metals are malleable, which means…
Pound or mold into shape
Brittle
Stretch into wire of 30

27. What do all elements in a group/family have in common?
Same # of Valence electrons
Same # of protons
Same # of rings/shells/energy levels of 30

28. ALKALI METALS-Group 1
So reactive that they are never found isolated in nature, only combined with other elements.

29. ALKALI METALS-Group 1 Characteristics Properties: Soft Shiny
One valance: electron makes them very reactive.

30. The Sodium in the class demo reacted so violently because it has…30
3 protons
1 neutron
2 valence electrons
1 valence electron

31. What family is Hydrogen in?
Alkali
Alkaline Earth
Halogens
No Family
0 of 30

32. Ca: important for bones.
Alkaline Earth Metals
Group 2 metals.
Very reactive, not as reactive as alkali metals due to having one more valence electron.
Ca: important for bones.

33. Metalloids Have some properties of both metals and nonmetals.
They are located on the zigzag line between the metals and the nonmetals.
Physical Properties:
Can be good at conducting electricity, therefore some are used as computer chips such as Si and Ge.

34. Non-metals Non metals lack properties of metals.
They are on the right side of the periodic table.
Non-metals O Fe
Fe2O3 = Iron Oxide = Rust
Non metals usually react with metals to make compounds.
In general, metals give up electrons to non-metals.

35. Properties of Metals cont…
Reactivity: Ability to react and combine with other elements. Some are more reactive than others. Sodium (Na) and potassium (K) are some of the most reactive metals.

36. Which of the following elements is most likely to react?
Chlorine
Helium
Iron of 30

37. What are the group 17 (7A) elements called?30
Alkaline Earth
Rare Earth
Halogen
Transition Metals

38. What is the Group/Family name of the elements in BLUE?30
Alkali
Alkaline Earth
Transition
Metalloids
Halogen
Noble Gas
Rare Earth

39. What is the Group/Family name of the elements in RED?30
Alkali
Alkaline Earth
Transition
Metalloids
Halogen
Noble Gas
Rare Earth

40. What is the Group/Family name of the elements in GREEN?30
Alkali
Alkaline Earth
Transition
Metalloids
Halogen
Noble Gas
Rare Earth

41. Predicting Reactions
Elements become more stable as they gain more valence electrons.
As a result, atoms will gain, lose or share electrons to form compounds so that they have 8 valence electrons or a full shell.
This is called the Octet Rule. However there are many exceptions, but this is an easy way to predict common reactions.

42. Atoms are “happy” when they have either
only 2 valence electrons (He) or 8
electrons.

43. Families of Non-metals
The Halogen family is group 17 (7A). Each element has 7 valence electrons, therefore it commonly takes one electron away from group one metals to make compounds.

44. Families of Non-metals
The Noble Gases are group 18 (8A). They have 8 valence electrons, therefore they are very stable and non-reactive.

45. Not a part of group 1. Generally found as H2 Hydrogen
It doesn’t fit into any other family because it is so different from all other elements.

46. Group 17 (7A) has 7 valence electrons and are called the30
Alkali metals
Alkaline Earth Metals
Halogens
Noble Gases

47. Group 18 (8A) has 8 valence electrons and are called30
Alkali metals
Alkaline Earth Metals
Halogens
Noble Gases

48. What element would Na (Sodium) bond with?30 Br K W Al

49. What element would Mg (Magnesium) bond with?30 Au Na Se Kr

50. How many Hydrogen atoms would bond to one N (Nitrogen)?6 2 8 3

51. Matter
Anything that has mass and takes up space

52. The four states of matter are solids, liquids, gasses and plasma.

54. Elements
Can’t be broken down into another substance.

55. The smallest particle of an element. Basic unit of all matter
Atom
The smallest particle of an element. Basic unit of all matter

56. An ELEMENT is a pure substance made up of only one type of atom.
Element vs. Compound
An ELEMENT is a pure substance made up of only one type of atom.
They may exist as atoms like the Noble Gases e.g. helium He or as molecules e.g. hydrogen H2 or sulfur S2

57. Compound EX: H20water CO2Carbon Dioxide C12022H11 Sugar
Chemical Combination of 2 or more DIFFERENT elements.
EX: H20water
CO2Carbon Dioxide
C12022H11 Sugar
C6H12O6 Glucose

58. A type of Molecule

59. chocolate

60. Theobromine, C7H8O4N2 or Chocolate
Formula
Ratio of atoms of each element in a compound.
Theobromine, C7H8O4N2 or Chocolate

61. Law of Conservation of Matter
Matter is neither created nor destroyed during a chemical change.
It recombines to make a new type of chemical.

62. Changes in Matter
Physical Change: When the state of matter changes.

63. Physical Change
whipping egg whites (air is forced into the fluid, but no new substance is produced)
magnetizing a compass needle (there is realignment of groups ("domains") of iron atoms, but no real change within the iron atoms themselves).
boiling water (water molecules are forced away from each other when the liquid changes to vapor, but the molecules are still H2O.)
dissolving sugar in water (sugar molecules are dispersed within the water, but the individual sugar molecules are unchanged.)
dicing potatoes (cutting usually separates molecules without changing them.)

64. Changes in Matter cont…
Chemical Change: When a substance(s) combines or decompose into a new substance.

66. Examples of a chemical change
iron rusting (iron oxide forms)
gasoline burning (water vapor and carbon dioxide form)
eggs cooking (fluid protein molecules uncoil and crosslink to form a network)
bread rising (yeast converts carbohydrates into carbon dioxide gas)
milk souring (sour-tasting lactic acid is produced)
suntanning (vitamin D and melanin is produced)

67. Both physical and chemical change5
Chemical change only
Physical change only
Both physical and chemical change

68. Both physical and chemical change5
Chemical change only
Physical change only
Both physical and chemical change

69. He, O2, N2, and Ne are all: 5
Atoms
Elements
Compounds

70. 5
Atoms
Elements
Compounds/molecules

71. H2, H2O, N2, and NaCl are all: 5
Atoms
Elements
Compounds
Molecules

72. 5
H, O, Na, Cl and C
H2O, NaCl and CO2

73. 30
Chemical change
Destroying matter
Physical change

74. A different substance with different properties30
A change in state
A different substance with different properties
No new substance

75. Both a chemical and a physical change30
Chemical change
Physical change
Both a chemical and a physical change

76. Characteristic Properties
Regardless of state of matter, a substance has a unique characteristic property.

77. Chapter 3 sections 1 and 3

78. Definite Shape and Definite Volume.

79. Molecules are packed closely together and slightly vibrate.

80. Very large molecules made of a chain of smaller molecules
Polymers form when chemical bonds link large numbers of monomers in a repeating pattern.

81. The properties of synthetic polymers make them ideal starting materials for many common objects.

82. Takes the shape of the container that it’s in.

83. Atoms and/or molecules are loosely packed together.

84. A mixture where particles can be seen and easily separated.
Examples: Milk, salad dressing and muddy water

85. The resistance of a liquid to flow.
The higher the viscosity, the slower it will flow.
Usually amorphic solids.

86. Have no definite shape and no definite volume.
Very compressible.

87. Particles are not touching, therefore the Intermolecular forces are broken.
Movement is random and independent of each other.

88. What are Galaxies? They are large groups of stars
There are billions of stars in a galaxy

89. Types of Galaxies

90. There are 3 main types of galaxies
Spiral: it has a nucleus
Irregular: it has not specific shape
Elliptical: it is a bright ball and is generally older

91. Our Galaxy It contains over 100 billion stars
It is about 100,000 light-years in diameter and 10,000 light-years thick