Name _____ _______________
Period ___________
Study Guide for Unit 1 Test Enriched 8 Science
Use NOS pages 12-16 in the beginning of the book as well as chapter 7 in your textbook, all lessons. These are
pages 231-260. You can also look in Chapter 9 pages 313-322 about the atom and Chapter 8 pages 273-278
about states of matter. You should know the parts of the atom, but you don’t need to know the scientists
who discovered each part.
METRIC
KHDbdcm prefixes and meanings King henry died by drinking chocolate milk
Kilo Hecto Deka base deci centi milli
Conversions using factor label method how many seconds are in 3 hours, 4 min. & 8 sec. (11,048 sec)
Accuracy vs. Precision- accuracy is how close to the “right” answer you are; precision is how consistent you are
Significant Figures (rules and operations) know rules and operations; 0.020 ml = 2 sig figs; + or – count
decimal places, mult./divide count sig figs; all non zero numbers are significant, place holder zeros are NOT;
zeros in between two sig. figs are; zeros to the right after a sig fig ARE significant.
Scientific Notation
Mass amount of matter in an object
Lab Tools and Units
TBB grams
Volume amount of space an object takes up Lab Tools and Units GRADUATED CYLINDER mL or cm3
MATTER (define)
Atom- smallest part of an element with all properties of that element
Structure of the Atom Nucleus (protons & neutrons), electron cloud has energy levels and electrons are there
Proton positive particle of the atom, found in the nucleus, has a mass of 1 amu
Neutron neutral (no charge) particle of the atom, found in the nucleus, has a mass of 1 amu
Electron negative particle of the atom, found in the electron cloud outside the nucleus, has
essentially no mass.
Chemical symbols (rules/examples) Only 1 or 2 letters, first letter must be capital ex: H or Au
Atomic number defines the element, is the number of protons. In a neutral atom, there is the
same number of electrons.
Mass number the mass of the atom, is equal to the number of protons plus the number of
neutrons.
Symbol
Au
Na
Atomic #
79
11
Mass #
197
23
Protons
79
11
Neutrons
118
12
Electrons
79
11
Pure Substances(definitions and examples)
Element simplest pure substance; made up of 1 kind of atom; Au, O2, He
Compound 2 or more elements chemically combined together H2O, NaCl, CO
Mixtures (define and give an example)
Homogenous 2 or more substances physically combined; looks same throughout; salt water,
Gatorade, air
Heterogeneous physical mixture of 2 or more substances that looks different throughout; trail
mix, chocolate chip cookie, fruit salad
PROPERTIES of MATTER (define and list)
Physical – characteristics that are observable and measurable. Nothing new is created !
Ex: color, size, shape, texture, odor, malleable, ductile, boiling/melting point, density, weight, mass,
volume, cutting, etc.
Chemical – characteristics that can change the substance to something new. The substance can:
Ex: burn, fizz, bubble, producte gas, react with water, acid, oxygen, change temperature
CHANGES OF MATTER (define and list)
Physical – substance changed its: shape, color, mass, weight, volume, etc.; ripping the paper, melting
chocolate
Chemical – The substance is: burning, fizzing, bubbling, producing gas, reacting with water, acid, oxygen,
having a change in temperature; burning paper, baking a cake,
STATES OR PHASES OF MATTER
Solid
particles fixed in place, definite shape and volume
Liquid
Particles can move and slide past one another, no definite shape, definite volume
Gas
(think wood block)
particles are free to move wherever they want, no definite shape or volume (think balloons)
(think water)