Chapter 6Section 1
1. atoms – basic unit of matter
2. nucleus - at the center of the atom; contains proton and neutrons
3. electron –part of an atom, located in energy levels, e-
4. isotope – atoms of the same element that have the same number of p+ and e- but different number of n0
5. compound – formed when 2 or more different elements combine
6. ionic bond – bond formed when one or more electrons are transferred from one atom to another
7. ion – atom that has a positive or negative charge because they have lost or gained 1 or more e-
8. covalent bond –bond formed by the sharing of electrons between atoms
9. molecule –compound in which the atoms are held together by covalent bonds.
10. van der Waals forces – a slight attraction that develops between the oppositely charged regions of nearby molecules
11. element – substance consisting entirely of one type of atom
12. neutron – part of an atom, located in nucleus, n0
13. proton – part of an atom, located in nucleus, p+
14. matter- anything that take up space and has mass
15. chemistry–study of matter
16. periodic table - a table of the chemical elements arranged in order of atomic number
Chapter 6 Section 2
1. chemical reaction –process that changes one set of chemicals into another set of chemicals by breaking and forming chemical bonds
2. physical change – changes appearance of the substance but not its composition
3. chemical change – anychangethat results in the formation of new chemicalsubstances caused by the making or breaking of bonds between atoms.
4. reactant – element or compound that enters into a chemical reactions
3. products – element or compound produced by a chemical reaction
5. coefficient – thenumbers placed before the reactants in a chemical equation so that the number of atoms in the products on the right side of the equation are equal to the number of atoms in the reactants on the left side.
6. subscript - number that is written below the element that lets you know how many molecules of that element are present
7. arrow in chemical equation means “yields” or “make”s or reacts to form
8. Law of conservation of mass –since mattercanneitherbecreatednorbedestroyed,a chemical equation must balance
9. endothermic reaction - reaction in which the system absorbsenergy from its surroundings; usually in the form of heat.
10. exothermic reaction – chemicalreactionthat releases energy by light or heat.
11. activation energy – energy needed to get a reaction started
12. catalyst –substance that speeds up the rate of a chemical reaction
13. enzyme – protein that acts as a biological catalyst
14. active site – specific place where a substrate binds on an enzyme
15. substrate – reactant of an enzyme-catalyzed reaction
Chapter 6 Section 3
1. polarity- the characteristic of some molecules that have 2 opposite poleswith an unequaldistribution of charges.
2. hydrogen bond – a weak interaction involving a hydrogen atom and another atom held together by a van
der Waals force.
3. cohesion-attraction between molecules of the same substance
4. adhesion-an attraction between molecules of different substance.
5. mixture - combination of two or more substances in which each substance retains its individual characteristics because they do not combine chemically.
6. homogenous mixtures- even composition of the substances throughout the mixture
7. solution – mixture where one of the substances dissolves in the other and these substances are even throughout; made up of a solvent and solute; another name for a homogeneous mixture
8. solvent – substance in which a solute is dissolved to form a solution
9. solute – substance that is dissolved in a solvent to make a solution
10. heterogenous mixtures –in a mixture, the components remain distinct from each other; they can be seen individually
11. homogenous mixtures-in a mixture, the components are uniform in composition throughout the mixture; they retain physical properties but can’t be separated
12. suspension–a heterogeneous mixture in which the particles settle out over time.
13. colloid - heterogeneous mixture in which the particles do not settle out over time.
14. acids- substances that release hydrogen ions (H+) when dissolved in water; pH values lower than 7.
15. bases - substances that release hydroxide ions (OH–) when dissolved in water
16. pH - the measure of concentration of H+ (hydrogen Ion)in a solution
17. H+ - the positively charged nucleus of hydrogen, H, without its electron; concentration of H+ determine the pH of substances
18. dissociation - the splitting of a molecule into smaller molecules, atoms, or ions, especially by a reversible process
19. buffers - mixtures that can react with acids or bases to keep the pH within a particular range
Chapter 6 Section 4
1. Monomers – small molecules that can join with other small molecules to make larger molecules
2. polymers – the larger molecules made up of monomers
3. macromolecule – giant molecules made of hundreds or thousands of smaller molecules
4. Polymerization- process of making macromolecules/polymers by joining smaller compounds together
5. Dehydration Synthesis- A chemical reaction involved in losing water molecule to join monomers to make a polymer
6.saccharide – sugar
7. monosaccharide – 1 sugar molecule
8. carbohydrates – macromolecule that occurs in living tissues or food and that can be broken down into energy by people or animals; made up of monomer monosaccharide; contains elements C, H, O
9. Disaccharides –carbohydrate made by joining 2 monosaccharides.
10. Polysaccharides -carbohydrate made by joining many monosaccharides.
11. starch - polysaccharide that functions as a carbohydrate storage unit and is an important constituent of the human diet
12. Cellulose – polysaccharide in plants that provides structural support in cell walls
13. Chitin – polysaccharide in hard outer shells of shrimp, lobsters, and some insects.
14. Glycogen – polysaccharide energy storage form of glucose found in animals
15. Lipid – macromolecule compounds that are oily to the touch and insoluble in water because they are nonpolar. Monomers are fatty acids joined to glycerol molecules
16. Nonpolar- describes a molecule that has equal charges all over the molecule; causes the molecule to not mix well with other substances; lipids are nonpolar
17. Phospholipids –substance made up of phosphate groups and lipids; found in the cell membrane
18. Proteins- macromolecules made up of amino acids; essential part of all living organisms, especially as structural components of body tissues such as muscle, hair, collagen, etc., and as enzymes and antibodies.
19. Amino acids – monomer for proteins; made up of a central carbon, a hydrogen, an amino group and a carboxyl group and an R group.
20. nucleic acid - substance present in living cells, especially DNA or RNA, whose molecules consist of many nucleotides linked in a long chain.
21. Nucleotide – monomer for nucleic acid; made up of one sugar, one nitrogenous base, and one phosphate
22. DNA- type of nucleic acid that stores and communicates genetic information
23. RNA – type of nucleic acid that carries information from DNA to the cell; helps with protein synthesis
24. ATP – type of nucleic acid that is used by cells to store and transport energy