1. Inorganic Chemistry Review

2. Matter
Anything that has
mass and volume
and takes up space.

3. There are 3 major states of matter
Solid
Liquid G s a

4. Tightly packed; usually regular pattern
SOLID
Tightly packed; usually regular pattern
Vibrate, but generally don’t move from place to place

5. Close together; usually no regular arrangement
Liquid
Close together; usually no regular arrangement
Vibrate; move about; slide past each other

6. Well separated; no regular arrangement Vibrate and move freely at
high speeds.

7. Composition of Matter
Matter - Everything in universe is composed of matter
Matter is anything that occupies space or has mass
Mass – quantity of matter an object has
Weight – pull of gravity on an object

8. Elements
Pure substances that cannot be broken down chemically into simpler kinds of matter
More than 100 elements (92 naturally occurring)

9. 90% of the mass of an organism is composed of 4 elements (oxygen, carbon, hydrogen and nitrogen)
Each element unique chemical symbol
Consists of 1-2 letters
First letter is always capitalized

10. Atoms
The simplest particle of an element that retains all the properties of that element
Properties of atoms determine the structure and properties of the matter they compose
Our understanding of the structure of atoms based on scientific models, not observation

11. The Nucleus Central core
Consists of positive charged protons and neutral neutrons
Positively charged
Contains most of the mass of the atom

12. The Protons
All atoms of a given element have the same number of protons
Number of protons called the atomic number
Number of protons balanced by an equal number of negatively charged electrons

13. The Neutrons
The number varies slightly among atoms of the same element
Different number of neutrons produces isotopes of the same element

14. Atomic Mass Protons & neutrons are found in the nucleus of an atom
Protons and neutrons each have a mass of 1 amu (atomic mass unit)
The atomic mass of an atom is found by adding the number of protons & neutrons in an atom
# of protons + # of neutrons =atomic mass

15. The Electrons
Negatively charged high energy particles with little or no mass
Travel at very high speeds at various distances (energy levels) from the nucleus
Are located around the nucleus

16. Periodic Table
Elements are arranged by their atomic number on the Periodic Table
The horizontal rows are called Periods & tell the number of energy levels
Vertical groups are called Families & tell the outermost number of electrons

18. Compounds Most elements do not exist by themselves
Readily combine with other elements in a predictable fashion

19. A compound is a pure substance made up of atoms of two or more elements
The proportion of atoms are always fixed
Chemical formula shows the kind and proportion of atoms of each element that occurs in a particular compound

20. Molecules are the simplest part of a substance that retains all of the properties of the substance and exists in a free state
Some molecules are large and complex

21. Chemical Formulas
Subscript after a symbol tell the number of atoms of each element
H20 has 2 atoms of hydrogen & 1 atom of oxygen
Coefficients before a formula tell the number of molecules
3O2 represents 3 molecules of oxygen or (3x2) or 6 atoms of oxygen

22. The tendency of elements to combine and form compounds depends on the number and arrangement of electrons in their outermost energy level
Atoms are most stable when their outer most energy level is filled (when it has 8 electrons)

23. Most atoms are not stable in their natural state
Tend to react (combine) with other atoms in order to become more stable (undergo chemical reactions)
In chemical reactions bonds are broken; atoms rearranged and new chemical bonds are formed that store energy

24. End of
Day One
Notes ? 

25. Covalent Bonds
Formed when two atoms share one or more pairs of electrons

26. Covalent Bonding In a COVALENT bond Electrons are shared between atoms
The number of shared atoms depends on how many are need to fill the octet rule

27. Chlorine
forms a
covalent
bond
with
itself
Cl2

28. How
will
two
chlorine
atoms
react? Cl Cl

29. Cl Cl Each chlorine atom wants to
gain one electron to achieve an octet

30. Cl Cl do to achieve an octet? What’s the solution – what can they
Neither atom will give up an electron –
It’s too close to filling the octet.
What’s the solution – what can they
do to achieve an octet?

31. Cl Cl

32. Cl Cl

33. Cl Cl

34. Cl Cl

35. Cl Cl
octet

36. Cl Cl octet circle the electrons for each atom that completes
their octets

37. Cl Cl The octet is achieved by each atom sharing the
electron pair in the middle
circle the electrons for
each atom that completes
their octets

38. Cl Cl The octet is achieved by each atom sharing the
electron pair in the middle
circle the electrons for
each atom that completes
their octets

39. Cl Cl This is the bonding pair circle the electrons for
each atom that completes
their octets

40. Cl Cl It is a single bonding pair circle the electrons for
each atom that completes
their octets

41. Cl Cl It is called a SINGLE BOND circle the electrons for
each atom that completes
their octets

42. Single bonds are abbreviatedCl Cl
Single bonds are abbreviated
with a dash
circle the electrons for
each atom that completes
their octets

43. This is the chlorine molecule,Cl Cl
This is the chlorine molecule,
Cl2
circle the electrons for
each atom that completes
their octets

44. O2
Oxygen is also one of the diatomic molecules

45. O
How will two oxygen atoms bond?

46. O
Each atom has two unpaired electrons

47. O

48. O

49. O

50. O

51. O

52. O

53. O Oxygen atoms are highly electronegative.
So both atoms want to gain two electrons.

54. O Oxygen atoms are highly electronegative.
So both atoms want to gain two electrons.

55. O

56. O O

57. O O

58. O O

59. Both electron pairs are shared.

60. O O
6 valence electrons
plus 2 shared electrons
= full octet

61. O O
6 valence electrons
plus 2 shared electrons
= full octet

62. O O
two bonding pairs,
making a double bond

63. O O =
For convenience, the double bond
can be shown as two dashes.

64. This is the oxygen molecule,=
this is so cool!!
This is the oxygen molecule, O2

65. Ionic Bonds Some atoms become stable by losing or gaining electrons
Atoms that lose electrons are called positive ions

66. F K Ionic Bonds In an IONIC bond, electrons are lost or gained,
resulting in the formation of IONS in ionic compounds. F K

67. K F

68. K F

69. K F

70. K F

71. K F

72. K F

73. + _ K F

74. + _ K F

75. K F _ + The ionic bond is the attraction between the positive K+ ion
and the negative F- ion

76. Atoms that gain electrons are called negative ions
Because positive and negative electrical charges attract each other ionic bonds form

77. Summary
Atoms want to have 8 electrons in their outer shell, so they will react to other atoms to get 8 electrons
Covalent bonds= two or more atoms SHARING electrons
Ionic Bonds= When one atom STEALS electrons from another, then there will be a positive and a negative ion which become attracted to each other

78. Questions?