1. Chemistry

2. What is Matter
Anything that has mass and volume

3. Atoms Atom: the basic unit of matter.
Subatomic particles: neutrons, electrons, and protons.

4. Subatomic Particles Protons (+) and Neutrons Electrons (-) Nucleus
Same mass
Electrons (-)
In the electron cloud in constant motion
Less mass
Electron –
Proton +
Neutron

5. Elements
Element: pure substance that consists of only one type of atom.
1 or 2 letter symbol
Atomic Number: # of protons
Atomic Mass: # of protons + neutron. 6 C
12.011

7. Isotopes atom with a different number of neutron ID by atomic mass
same chemical properties
unstable nucleuses  give off radiation
scientific testing, cancer therapy, and to date objects

8. Compounds
Compound: the combination of two or more elements,; water, glucose, and methane
Atoms are held together by chemical bonds.
Smallest unit of a compound is a molecule.
H2O C6H12O6 CH4

9. Types of Chemical Bonds
Ionic Bonds
Covalent Bonds

10. Ionic Bond The transfer of an electron from one atom to another atom.
Ions: positively and negatively charged atom.
Positively charged atoms lose electrons.
Negatively charged atoms gain electrons.
F K+ S2-

11. Ionic Bond

12. Covalent Bonds
The linkage of two atoms by the sharing of two electrons.
Permits each atom to have a stable closed-shell electron configuration.
Molecule: combination of two or more atoms

13. Covalent Bond

14. Formulas
Chemical Formula: represents the number and types of atoms in a molecule
H2O, CaO, H2SO4
Structural Formula: represent how atoms are joined and arranged in various models
Single line: single bond
Double line: double bond

15. Chemical Reactions
Synthesis: 2 or more atoms, the reactants react to form a product
A + B  AB
Decomposition: reactant molecule breaks into simple molecule or atoms
AB  A + B
Exchange Reaction (Replacement): reactants exchange partners
AB + CD  AD + CB

16. Reactions
Reversible Reaction: products of reaction can change back into the reactants
Double Arrow: A + B ↔ AB
Catalyst: a molecule or atom that increases reaction rate without being changed by the reaction

17. Acids and Bases
Electrolyte: compounds that release ions in water and conduct electricity
NaCl  Na+ + Cl-
Acids: release H+
HCl  H + + Cl-
Bases: release OH-
NaOH  Na+ + OH-

18. pH A logarithmic scale that measures the concentration of H3O+
Neutral: 7
Acidic: < 7
Basic or Alkaline: > 7

20. Chemical Constituents of Cells

21. Organic vs. Inorganic Organic: compounds containing C and H
Nonelectrolytes: don’t dissolve in water as ions
Don’t conduct electricity
Inorganic: compounds that don’t contain C
Electrolytes: dissolve in water as ions
conduct electricity

22. Inorganic Substances Water: universal solvent
Oxygen: used to release energy from sugar
Carbon Dioxide: cellular metabolism byproduct
Salts: abundant in tissues and fluids
Na+, Cl-, K+, Ca2+, Mg2+, PO43+
Transport, muscle contraction, and nerve impulses

23. Organic Substances Carbohydrates: energy source C, H, O (CH2O)n
Stored as energy reserves
Building materials
Monomer: monosaccaride
glucose, fructose
Polymer: disaccarides or polysaccarides
Glycogen, sucrose

24. Lipids C, H, O C57H110O6 Fatty Acids and Glycerol
Fats, Oils, Waxes, and Steroids
Insoluble in water
Fats: energy storage

25. Triglyceride

26. Lipids Saturated: maximum no. of H No double bonds
Unstaturated: less than the maximum no. of H
Double bonds

27. Proteins C, H, O, N Structural material, energy sources, and enzymes
Enzymes: catalysts
Protein: made up of amino acids
20 different amino acids in nature
Function depends on order of amino acids and how it is folded

28. Protein

29. Nucleic Acids C, H, O, N, P Compose DNA and RNA Monomer: nucleic acid
Genetic material
Monomer: nucleic acid
5-sugar, phosphate group, nucleotide

30. DNA