1. Chemistry and the Properties of Life

2. Properties of Life Cellular Organization Homeostasis Metabolism
Responsiveness
Reproduction
Heredity
Growth
Movement

3. Cellular Organization
All living things are made of cells.

4. Homeostasis
All organisms maintain stable internal conditions that are different than the surrounding environment.

5. Metabolism All organisms require energy and produce waste products.
Food energy is used to maintain internal order and to grow.

6. Responsiveness
All organisms respond to internal and external stimuli.

7. Reproduction
All organisms are capable of reproduction

8. Heredity
Any organism originates from an organism or organisms of the same species.
Living things do not spring into life randomly.

9. Growth All organisms grow and develop through definite stages
Beginning, growth, maturity, decline, and death.

10. Movement
All organisms are capable of self-generated movement at some scale and at some stage of their life cycle.

11. Chemistry Basics All living things are made of atoms
Atoms: the smallest particle into which an element can be divided and still be the same substance

12. Subatomic Particles
Protons: positively charged particles located in the nucleus
Neutrons: particles without a charge that are located in the nucleus
Electrons: negatively charged particles that are located in the electron cloud

13. Electron Configuration
The location within the electron cloud where the electrons are most likely to be found
1st shell holds maximum of 2 electrons
All other shells hold a maximum of 8 electrons

14. Atomic Structure

15. Elements on the Periodic Table

16. Atomic Weight
The total number of protons and neutrons added together

17. Periodic Table

18. How to find numbers of… Number of protons = Atomic Number
Number of electrons = Atomic Number
Number of neutrons =
Atomic Weight – Atomic Number
*Round atomic weight to the nearest whole number before subtracting

19. Outer Shells
The number of outer shells an atom has in its electron cloud can be determined by the row the element is placed on the periodic table

20. Valence Electrons
The number of valance electrons an atom has can be determined by which column the element is placed into on the periodic table

21. Shells and Valances

22. Bonding to Make Compounds

23. Molecule
A group of atoms held together by covalent bonds

24. Compound
A substance composed of two or more elements that are combined

25. Valance Electrons The number of electrons in the outer shell.
Used for bonding

26. Octet Rule
When bonding, each atom wants to have a full outer shell (8 valance electrons)
***Exception is Hydrogen, which can only hold two electrons in its outer shell

27. Types of Bonding
Covalent Bonding
Ionic Bonding
Hydrogen Bonding

28. Covalent Bonds
When bonds form between atoms by sharing valence electrons

29. Ionic Bonds
When bonds form between atoms by either gaining or losing electrons
Results in the compound having either a positive or negative charge

30. Ions When an atom has an electrical charge it is called an ion
If an atom gains an electron it has a negative charge
If an atom loses an electron it has a positive charge

31. Polarity
When shared electrons are attracted to one atom more strongly than another, so it has a slightly negative charge
The other atom that the electrons are less strongly attracted to has a slightly positive charge

32. Solubility Like dissolves like
Substances with like charges will dissolve one another, but substances with opposite charges will not

33. Hydrogen Bond
When a hydrogen atom has a partial positive charge that is very strong it attracts to the negative pole of specific other molecules
Oxygen, Nitrogen, Fluorine
This is a very strong bond, but not as strong as a covalent bond.