Chapter 2 and 5.1

• Matter is anything that has mass and takes up space.
• Atom: the smallest particle of a chemical element that can exist.
• Electron: a stable subatomic particle with a charge of negative electricity, found in all atoms and acting as the primary carrier of electricity in solids.
• Proton: a positively charged subatomic particle found in the nucleus of an atom.
• Neutron: a neutral (uncharged) subatomic particle found in the nucleus of an atom.
• Element: a substance made up of only one kind of atom.
• Compound: a substance composed of two or more different elements chemically combined together.
• Atomic Mass: The average mass of an atom of an element.
• Atomic Number: The number of protons in an atom.
• Isotopes: Atoms of the same element that have different numbers of neutrons.
• Molecule: A group of atoms held together by chemical bonds.
• Electronegativity is the ability of an atom to attract electrons
• How are atoms structured?

  Atoms are structured with a nucleus containing protons and neutrons, surrounded by electrons in energy levels.
• Polar covalent bonds are when electrons are shared unequally between atoms.
• Non-polar covalent bonds are weak and do not conduct electricity. (“no poles”)
• Ionic bonds are formed when a metal loses electrons to form a positively charged ion
• Hydrogen bonds are weak bonds between the hydrogen atoms of adjacent molecules.
• Hydrogen bonds give water special properties of adhesion, cohesion, and surface tension
• Cohesion is the attraction of water molecules to one another (water beads up on leaves).
• Surface tension is the force that holds together the surface layer of liquid (a drop of water has a curved shape due to its own weight).
• Anion is when a element gains electrons and becomes negatively charged
• Cation is a positively charged ion that has gained electrons and is attracted to the anode
• Synthesis Reaction is the reaction in which two or more reactants combine to form one or more products.
• Decomposition Reactions are reactions where one compound breaks down into simpler compounds.
• Exchange reactions are reactions that involve the transfer of electrons between two molecules.
• Endothermic reactions are reactions that require energy to take place.
• Exothermic reactions release energy from the bonds of the reactants.
• Endergonic reactions are reactions that require energy to break bonds and are spontaneous
• Exergonic reactions are reactions that require energy to break bonds.
• Anabolic reactions are reactions that build up molecules from simpler ones.
• Catabolic reactions are reactions that break down molecules into smaller molecules.
• Specific Heat is why water is able to stay fluid in wide range of temps and take along to time to heat and cold down.
• Water is the universal solvent
• Solute is the substance that is dissolved in a solution.
• Solvent is the liquid that dissolves the solute. It is the liquid that the solute is dissolved in.
• 1-6 pH is acidic
• 7 pH is netural (pure water)
• 8-14 pH is basic/alkaline
• The pH logarithmic scale is by 10x each time you move on the scale
• The four major macromolecules are Lipids, Carbohydrates, Proteins, and Nucleic Acids