1. Chemistry of Life
Inorganic Chemistry

2. Elements
A chemical element is a pure substance that consists entirely of one type of atom.
92 elements occur naturally.
96% of the mass of a human is made up of Carbon, Hydrogen, Oxygen, and Nitrogen.
C stands for carbon.
H stands for hydrogen
O stands for oxygen.
N stands for nitrogen
Na stands for sodium.
Cl stands for chlorine.
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3. The study of chemistry begins with the basic unit of matter, the atom.
Atoms
The study of chemistry begins with the basic unit of matter, the atom.
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4. Atoms contain subatomic particles that are even smaller.
Placed side by side, 100 million atoms would make a row only about 1 centimeter long.
Atoms contain subatomic particles that are even smaller.
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5. The subatomic particles that make up atoms are Protons (+)
Neutrons (0)
Electrons (-)
Electrons
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Protons and Neutrons

7. The number of protons in an atom of an element is the element's atomic number
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8. Mass number is the number of protons and neutrons in the nucleus of an atom

9. Examples

10. Atoms of the same element that differ in the number of neutrons they contain are known as isotopes.
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11. Because they have the same number of electrons, all isotopes of an element have the same chemical properties.
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12. A chemical compound is a substance formed by the chemical combination of two or more elements in definite proportions.
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13. Chemical Bonds
The atoms in compounds are held together by chemical bonds.
The electrons that are available to form bonds are called valence electrons.
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15. Lewis Dot Structure A way of representing atoms or molecules by showing electrons as dots surrounding the element symbol. One bond is represented as two electrons.

16. The main types of chemical bonds are: ionic bonds covalent bonds
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17. Covalent Bonds Sometimes electrons are shared by atoms instead of being transferred.
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18. A covalent bond forms when electrons are shared between atoms.
single covalent bond
double bond
triple bond
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19. The structure that results when atoms are joined together by covalent bonds is called a molecule.
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20. Ionic Bonds
An ionic bond is formed when one or more electrons are transferred from one atom to another.
These positively and negatively charged atoms are known as ions.
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21. Summary of Chemical Bonds
Ionic Bonds
Covalent Bonds
Form ions
Gain or lose electrons
Fill outer shell
Combine metals & nonmetals
Form molecules
Share electrons
Fill outer shell
Combine two nonmetals

22. Examples of Ionic and Covalent Compounds
NaCl
CaCl₂
MgF₂
Ca₃(PO₄)₂
MgS
CaCO₃
H₂O
NH₃ H₂
CH₄
C₆H₁₂O₆
C₆H₆

23. Solutions and Suspensions
A mixture is a material composed of two or more elements or compounds that are physically mixed but not chemically combined.
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24. Examples of Mixtures

25. Two types of mixtures can be made with water solutions suspensions
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26. Solutions
All the components of a solution are evenly distributed throughout the solution.
solute—the substance that is dissolved.
solvent—the substance in which the solute dissolves.
Water is the UNIVERSAL SOLVENT because it can dissolve many substances
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27. Example of parts of a solution
Lemonade =solution
Solvent = water
Solute = sugar/lemon juice

28. Acids, Bases, and pH
A water molecule is neutral, but can react to form hydrogen and hydroxide ions.
H2O   H+ + OH-
pH – measure of how acidic or basic a solution is
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29. The pH scale 
Chemists devised a measurement system called the pH scale to indicate the concentration of H+ ions in solution.
The pH scale ranges from 0 to 14.
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30. Acid below 7; more H+ than OH- Base above 7; less H+ than OH-
The pH Scale
At a pH of 7, the concentration of H+ ions and OH- ions is equal - Neutral
Acid below 7; more H+ than OH-
Base above 7; less H+ than OH-
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The concentration of H+ ions determines whether solutions are acidic or basic.

31. Properties of Water
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32. A water molecule is polar because there is an uneven distribution of electrons between the oxygen and hydrogen atoms.
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33. Hydrogen Bonds
Because of their partial positive and negative charges, polar molecules can attract each other.
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34. Cohesion is an attraction between molecules of the same substance.
Because of hydrogen bonding, water is extremely cohesive.
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35. Adhesion is an attraction between molecules of different substances.
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36. Non-polar molecule – electrons are equally shared by atoms

37. Characteristics of Water
Water is polar
Water resists temperature changes
Water expands when it freezes
Water is cohesive – it sticks to itself
Water is adhesive – it sticks to other stuff
Water makes up 60-80% of living organisms