Chemistry Fall 2013 Review

Box 1: Chapter 1 Scientific method Fold the sheet of paper into 4 squares. Give each box a chapter name: Box 1: Chapter 1 Scientific method Box 2 : Chapter 3- Properties of matter Box 4: Chapter 3_ Mixture and compoiunds Box 5 : Chapter 4Structure of the atom Chapter 6: Chapter 4 Isotopes Box 7: Chapter 5 Atomic emission/ flame test Box 8: Chapter 6The periodic table and periodic law

Chapter 1 and 2 Density= mass / volume Temperature is a measurement of the average kinetic energy of the particles that make up an object. Increase in K.E. can result in melting. ( Review notes and powerpoint to add any additional information here)

Chapter 3 3 states of matter: Solid: (s)definite shape and definite volume Has least random molecular motion Particles in a rigid and fixed pattern (tightly packed) Strongest attractive force Liquid: (aq) or (l) no definite shape, definite volume Stronger attractive force than gas, but weaker attractive force than a solid in the same conditions Gas: no definite shape and no definite volume Has greatest random molecular motion and energy Particles farthest apart Weakest attractive force

Chapter 3 Physical change vs Chemical Change Physical change: Examples: melting, evaporation, crystallization, dissolving, bending Chemical change: Examples: igniting, burning, corrosion, rusting, decomposing, fermenting, exploding.

Chapter 3 Endothermic vs Exothermic Endothermic: absorbs heat from surroundings. Example: melting an ice cube ( solid to liquid), evaporation Exothermic: releases heat to surroundings. Example: Liquid to solid Gas to liquid

Chapter 3 Two types of matter: 1. Pure substance : uniform and unchanging composition. 2 types: Elements and compounds - compounds: made up of 2 or more different elements that are chemically combined in a definite ratio. example of compound: NaCl example of element: Na 2. Mixture = Consists of 2 or more substances that can be physically separated. 2 types: -heterogenous -homogenous

Chapter 3 Separation techniques: Distillation- separates liquids based on their different boiling points. Example: alcohol and water Filtration – a technique that uses a porous barrier to separate a solid from a liquid.( when the solid does not dissolve in water) Example: sand and water

Chapter 4 Atom- smallest particle of an element Experiments about the history of the atom, led to the conclusion that an atom is mainly empty space, and the nucleus has a positive charge. The subatomic particles of an atom include protons, neutrons and electrons. The nucleus of the atom is made up of protons and neutrons. The electrons of an atom travel outside the nucleus in different orbitals. Define Heisenberg’s uncertainty principle

Neutron n ~1 Electron e- -1 Proton p +1 1 Particle Symbol Location Relative Charge Relative Mass Electron e- Outside nucleus traveling in orbitals -1 1/1840 ( relative mass of zero) Much smaller than protons and neurtons Proton p Inside nucleus +1 1 Neutron n ~1

Chapter 4 Mass number= # of protons + # of neutrons Number of neutrons= mass number – atomic number In a neutral atom, the # of protons equals the # of electrons.

Isotopes: Isotope Abundance: Chapter 4 Atoms that have the same number of protons but a different number of neutrons. Example: Rb-85 and Rb 87 ( the difference between them is there mass number) Isotope Abundance: The atomic mass is a weighted average of the masses of all of its naturally occurring isotopes. Most of the time it can also tells you which isotope is most abundant.

Chapter 5 The energy level of electrons in shells farther away from the nucleus have a greater amount of energy than those closer to the nucleus The color we see from fireworks and flame tests is due to electrons releasing energy when they drop to their ground state (lower energy).

Chapter 5 Electron configuration example: 1s22s22p63s23p64s23d8 Orbital diagram example:

Chapter 6 Metals vs Non-metals Metals: tend to lose electrons easily when bonding and form positive ions (cations). Good conductors of heat and electricity, malleable and ductile. Non-Metals: tend to gain electrons and form negative ions (anions). Poor conductors of electricity.

Chapter 6 Noble gases- group 8 elements, all have the most stable outer electron configuration Groups/families= vertical columns on periodic table All elements in the same group share similar properties (like a family) All have the same number of valence electrons Periods= rows on periodic table Represent energy levels

Chapter 7 Ionic bonding involves the transfer of electrons from the metal atom to the non-metal atom. Electrons are the subatomic particles that are involved with chemical bonding

Chapter 7 List examples of naming ionic compounds and writing formulas: Lewis dot diagrams with ionic compound example: