1. Part I: Atoms, elements and compounds

2. Matter:

3. Matter: the substance or substances of which any physical object is made

4. Matter: the substance or substances of which any physical object is made
All matter in the universe is made of 92 naturally occurring They cannot be broken down into simpler particles by chemical reactions. They are located on the periodic table.

5. Matter: the substance or substances of which any physical object is made
All matter in the universe is made of 92 naturally occurring elements . They cannot be broken down into simpler particles by chemical reactions. They are located on the periodic table.

6. Matter: the substance or substances of which any physical object is made
All matter in the universe is made of 92 naturally occurring elements . They cannot be broken down into simpler particles by chemical reactions. They are located on the periodic table.
Example:

7. Matter: the substance or substances of which any physical object is made
All matter in the universe is made of 92 naturally occurring elements . They cannot be broken down into simpler particles by chemical reactions. They are located on the periodic table.
Example: Oxygen

8. Matter: the substance or substances of which any physical object is made
All matter in the universe is made of 92 naturally occurring elements . They cannot be broken down into simpler particles by chemical reactions. They are located on the periodic table.
Example: Oxygen
The smallest particle of an element that has the properties of that element is an .

9. Matter: the substance or substances of which any physical object is made
All matter in the universe is made of 92 naturally occurring elements . They cannot be broken down into simpler particles by chemical reactions. They are located on the periodic table.
Example: Oxygen
The smallest particle of an element that has the properties of that element is an atom .

10. Matter: the substance or substances of which any physical object is made
All matter in the universe is made of 92 naturally occurring elements . They cannot be broken down into simpler particles by chemical reactions. They are located on the periodic table.
Example: Oxygen
The smallest particle of an element that has the properties of that element is an atom . A pure element is made of 1 type of atom.

11. Two or more elements that are chemically combined in definite proportions form a .
Example:

12. Two or more elements that are chemically combined in definite proportions form a compound .
Example:

13. Two or more elements that are chemically combined in definite proportions form a compound .
Example: water

14. Two or more elements that are chemically combined in definite proportions form a compound .
Example: water
The smallest particle of a compound that has the properties of that compound is a .

15. Two or more elements that are chemically combined in definite proportions form a compound .
Example: water
The smallest particle of a compound that has the properties of that compound is a molecule .

16. Two or more elements that are chemically combined in definite proportions form a compound .
Example: water
The smallest particle of a compound that has the properties of that compound is a molecule .
An abbreviation for an element is called a . The first letter is always capitalized
Example:

17. Two or more elements that are chemically combined in definite proportions form a compound .
Example: water
The smallest particle of a compound that has the properties of that compound is a molecule .
An abbreviation for an element is called a symbol. The first letter is always capitalized
Example:

18. Two or more elements that are chemically combined in definite proportions form a compound .
Example: water
The smallest particle of a compound that has the properties of that compound is a molecule .
An abbreviation for an element is called a symbol. The first letter is always capitalized
Example: O or He

19. Two or more elements that are chemically combined in definite proportions form a compound .
Example: water
The smallest particle of a compound that has the properties of that compound is a molecule .
An abbreviation for an element is called a symbol. The first letter is always capitalized
Example: O or He
An abbreviation for a compound is called a . This shows the number of atoms of each element found in one molecule.
Example:

20. Two or more elements that are chemically combined in definite proportions form a compound .
Example: water
The smallest particle of a compound that has the properties of that compound is a molecule .
An abbreviation for an element is called a symbol. The first letter is always capitalized
Example: O or He
An abbreviation for a compound is called a formula. This shows the number of atoms of each element found in one molecule.
Example:

21. Two or more elements that are chemically combined in definite proportions form a compound .
Example: water
The smallest particle of a compound that has the properties of that compound is a molecule .
An abbreviation for an element is called a symbol. The first letter is always capitalized
Example: O or He
An abbreviation for a compound is called a formula. This shows the number of atoms of each element found in one molecule.
Example: H2O

22. Part II: Structure of atoms
Key Idea: Each type of atom consists of three different subatomic particles in differing amounts.
Part II: Structure of atoms

23. Subatomic Particle
Charge
Mass
Location
Proton
Neutron
Electron

24. Subatomic Particle
Charge
Mass
Location
Proton +
Neutron
Electron

25. Subatomic Particle
Charge
Mass
Location
Proton + 1
Neutron
Electron

26. Subatomic Particle
Charge
Mass
Location
Proton + 1
Nucleus
Neutron
Electron

27. Subatomic Particle
Charge
Mass
Location
Proton + 1
Nucleus
Neutron
None
Electron

28. Subatomic Particle
Charge
Mass
Location
Proton + 1
Nucleus
Neutron
None
Electron

29. Subatomic Particle
Charge
Mass
Location
Proton + 1
Nucleus
Neutron
None
Electron

30. Subatomic Particle
Charge
Mass
Location
Proton + 1
Nucleus
Neutron
None
Electron -

31. Subatomic Particle
Charge
Mass
Location
Proton + 1
Nucleus
Neutron
None
Electron -

32. Subatomic Particle
Charge
Mass
Location
Proton + 1
Nucleus
Neutron
None
Electron -
Outside nucleus

33. Atomic number:
It also equals the number of
because an atom has a neutral charge. The positive protons cancel out the negative electrons.

34. Atomic number: the number of protons found in the nucleus
It also equals the number of
because an atom has a neutral charge. The positive protons cancel out the negative electrons.

35. Atomic number: the number of protons found in the nucleus
It also equals the number of electrons because an atom has a neutral charge. The positive protons cancel out the negative electrons.

36. Atomic number: the number of protons found in the nucleus
It also equals the number of electrons because an atom has a neutral charge. The positive protons cancel out the negative electrons.
Atomic mass:
To determine the number of neutrons in an atom, you should subtract the from the atomic mass.

37. Atomic number: the number of protons found in the nucleus
It also equals the number of electrons because an atom has a neutral charge. The positive protons cancel out the negative electrons.
Atomic mass: the number of protons + the number of neutrons
To determine the number of neutrons in an atom, you should subtract the from the atomic mass.

38. Atomic number: the number of protons found in the nucleus
It also equals the number of electrons because an atom has a neutral charge. The positive protons cancel out the negative electrons.
Atomic mass: the number of protons + the number of neutrons
To determine the number of neutrons in an atom, you should subtract the # of protons from the atomic mass.

39. Part III: Chemical bonding (makes compounds)
Key Idea: Atoms form bonds in order to fill their outer electron shell and become stable.
Part III: Chemical bonding (makes compounds)

40. Covalent Bonds
Definition: _____________________________ ______________________________________
Atoms form covalent bonds to try to fill their outer electron shell, or the ___________ shell
The number of covalent bonds an atom can form depends on the number of electrons in its outer shell, or the number of ___________ _________________.

41. Covalent Bonds
Definition: 2 atoms share electrons in an attempt to fill the outer electron shell
Atoms form covalent bonds to try to fill their outer electron shell, or the ___________ shell
The number of covalent bonds an atom can form depends on the number of electrons in its outer shell, or the number of ___________ _________________.

42. Covalent Bonds
Definition: 2 atoms share electrons in an attempt to fill the outer electron shell
Atoms form covalent bonds to try to fill their outer electron shell, or the valence shell
The number of covalent bonds an atom can form depends on the number of electrons in its outer shell, or the number of ___________ _________________.

43. Covalent Bonds
Definition: 2 atoms share electrons in an attempt to fill the outer electron shell
Atoms form covalent bonds to try to fill their outer electron shell, or the valence shell
The number of covalent bonds an atom can form depends on the number of electrons in its outer shell, or the number of valence electrons.

44. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen
Carbon
Oxygen
Nitrogen

45. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
Carbon
Oxygen
Nitrogen

46. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
Carbon
Oxygen
Nitrogen

47. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon
Oxygen
Nitrogen

48. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon
Oxygen
Nitrogen

49. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon
Oxygen
Nitrogen

50. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6
Oxygen
Nitrogen

51. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
Oxygen
Nitrogen

52. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell)
Oxygen
Nitrogen

53. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen
Nitrogen

54. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen
Nitrogen

55. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen 8
Nitrogen

56. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen 8
Nitrogen

57. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen 8
6 (2nd Shell)
Nitrogen

58. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen 8
6 (2nd Shell)
Nitrogen

59. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen 8
6 (2nd Shell)
Nitrogen

60. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen 8
6 (2nd Shell)
Nitrogen 7

61. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen 8
6 (2nd Shell)
Nitrogen 7

62. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen 8
6 (2nd Shell)
Nitrogen 7
5 (2nd Shell)

63. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen 8
6 (2nd Shell)
Nitrogen 7
5 (2nd Shell) 3

64. Complete the Chart Element Total # of Electrons
# of Electrons in the First Shell
# of Electrons in the Valence Shell
# of Electrons Needed for a Full Valence Shell
# of Covalent bonds it can form
Hydrogen 1
1 (1st Shell)
Carbon 6 2
4 (2nd Shell) 4
Oxygen 8
6 (2nd Shell)
Nitrogen 7
5 (2nd Shell) 3
*HONC – ; number of bonds each forms 

65. Examples Each line represents 1 bond
Both molecules have each electron making correct number of bonds so each atom is stable and happy 

66. Polar Covalent Bond Definition:
Oxygen and nitrogen are electron hogs and often form polar covalent bonds with the atoms they are bound to. They tend to have a partial negative charge. The other atom in the bond has a partial positive charge.

67. Polar Covalent Bond
Definition: a covalent bond where the atoms don’t share the electrons equally. One atom in the bond holds the electron closer.
Oxygen and nitrogen are electron hogs and often form polar covalent bonds with the atoms they are bound to. They tend to have a partial negative charge. The other atom in the bond has a partial positive charge.

68. Examples O H H

69. Examples O H H

70. Examples O H H

71. Nonpolar covalent bond
Definition:

72. Nonpolar covalent bond
Definition: the electrons shared by the adjacent atoms in the bonds are shared equally

73. Nonpolar covalent bond
Definition: the electrons shared by the adjacent atoms in the bonds are shared equally
Examples:

74. Nonpolar covalent bond
Definition: the electrons shared by the adjacent atoms in the bonds are shared equally
Examples:

75. Ionic Bond Definition: Ion- Can be positive ( electrons) or negative
Occurs because one atom wants to gain an electron to fill its valence shell so bad it will rip electrons away from another atom that wants to get rid of an electron so it can have a full valence shell.

76. Ionic Bond
Definition: Bond (attraction) between a positive ion and a negative ion
Ion-
Can be positive ( electrons) or negative
( electrons)
Occurs because one atom wants to gain an electron to fill its valence shell so bad it will rip electrons away from another atom that wants to get rid of an electron so it can have a full valence shell.

77. Ionic Bond
Definition: Bond (attraction) between a positive ion and a negative ion
Ion-atom that lost or gained an electron
Can be positive ( electrons) or negative
( electrons)
Occurs because one atom wants to gain an electron to fill its valence shell so bad it will rip electrons away from another atom that wants to get rid of an electron so it can have a full valence shell.

78. Ionic Bond
Definition: Bond (attraction) between a positive ion and a negative ion
Ion-atom that lost or gained an electron
Can be positive (lost electrons) or negative
( electrons)
Occurs because one atom wants to gain an electron to fill its valence shell so bad it will rip electrons away from another atom that wants to get rid of an electron so it can have a full valence shell.

79. Ionic Bond
Definition: Bond (attraction) between a positive ion and a negative ion
Ion-atom that lost or gained an electron
Can be positive (lost electrons) or negative (gained electrons)
Occurs because one atom wants to gain an electron to fill its valence shell so bad it will rip electrons away from another atom that wants to get rid of an electron so it can have a full valence shell.

80. Example

81. Example

82. Example

83. Practice
A fluorine atom has 9 protons and 10 electrons. Is it a neutral atom, a positive ion or a negative ion?
A nitrogen atom has 7 protons and electrons. Is it a neutral atom, a positive ion or a negative ion?
A calcium atom has 20 protons and 18 electrons. Is it a neutral atom, a positive ion or a negative ion?

84. Practice
A fluorine atom has 9 protons and 10 electrons. Is it a neutral atom, a positive ion or a negative ion? Negative  extra e-
A nitrogen atom has 7 protons and electrons. Is it a neutral atom, a positive ion or a negative ion?
A calcium atom has 20 protons and 18 electrons. Is it a neutral atom, a positive ion or a negative ion?

85. Practice
A fluorine atom has 9 protons and 10 electrons. Is it a neutral atom, a positive ion or a negative ion? Negative  extra e-
A nitrogen atom has 7 protons and electrons. Is it a neutral atom, a positive ion or a negative ion? Neutral  (+) = (-)
A calcium atom has 20 protons and 18 electrons. Is it a neutral atom, a positive ion or a negative ion?

86. Practice
A fluorine atom has 9 protons and 10 electrons. Is it a neutral atom, a positive ion or a negative ion? Negative  extra e-
A nitrogen atom has 7 protons and electrons. Is it a neutral atom, a positive ion or a negative ion? Neutral  (+) = (-)
A calcium atom has 20 protons and 18 electrons. Is it a neutral atom, a positive ion or a negative ion? Positive  2 extra p+

87. Hydrogen Bond
Definition:

88. Hydrogen Bond
Definition: attraction between 2 polar compounds; partial positive hydrogen in one molecule is attracted to partially negative oxygen or nitrogen in another molecule

89. Example