I. Define pure science and technology. Give an example of each. 

pure science: ecperimneting to learn more about the world EX. discovering a new star

technology: the application of science for practical uses EX.cell phones, computers

2. What is the difference between a scientific theory and a scientific law'? 

scientific law: a descriptive statement of equation that predicts events & describes nature

scientfic theory: ideals that ecplain related observations & is supported by a large body of scientific evidence

** laws describe how something works; theories ecplain why something happens

3. Distinguish between a hypothesis and a theory. 

hypothesis: testable statement/question/educated guess

theory: explanation based on experimentation after you've run many experiments

4. Describe the steps in the scientific method. 

series of logical steps to solve problems:

purpose/question

research

hypothesis

experiment

analysis data

draw your conclusion

poster on wall

temp: kelvin

mass: kilogram

length:meter

time:second

6. Convert the following: 1.55 m = ___ cm                0.545 L = ___ mL     

155cm

545ml

.35hg

.454kg

.01997dg

3.25x10^8m

2.4x10^negative 6s

9. Define element and compound. 

Element: An element is a pure substance that cannot be broken down into any simpler substances by chemical methods.

compound: A chemical compound is a pure chemical substance consisting of two or more different chemical elements that can be separated into simpler substances by chemical reactions.

Name and                   describe the 4 states of matter. 

solid

liquid

gas

plasma

solid: paricles are close togetger and have only enough energy to vibrate in place. have definate volume

liquid: particles have enough energy to move out of arangment and flow past each other have definite volume, and flow to the shape of their container

gas: particles have enough energy to break free of each other and move in all directions have indefinite shape and volume

plasma: free moving ions and electons

the kinetic theory states all matter is matter is made up of small particles in constant motion.

the higher the temp the faster they move, and at the same temp, heavier particles move slower than lighter particles

. Define evaporation, condensation, melting, sublimation, and freezing. 

evaporation: Evaporation is the process whereby atoms or molecules in a liquid state (or solid state if the substance sublimes) gain sufficient energy to enter the gaseous state.

condensation: 

Give 3 examples of physical properties. 

color

shape

density

melting point

14     When do you use a line graph'? Pie graph? Bar graph?

line graph: shows changes over time

pie graph: shows parts of a whole

bar graph: used to compare things in different grorps

14     Where are the independent and dependent variables plotted on a line graph'? 

independent: x

dependent: y

Find the density of a rock with a mass of 119 grams and a volume of 14 cm³. 

density= m/v

119/14

8.5=d

Give 3 examples of physical changes and 3 examples of chemical changes. 

physical changes: tearing paper, boiling a liquid, melting ice.

chemical changes: burning, rusting, & all chemical reactions, neutralization of an acid

. What particles are located in the nucleus'? What is the charge on the nucleus'? 

protons & neutrons

nucleus has a positvie charge

electron cloud has an negative charge

19. Why do atoms have no electric charge'? 

bc the # of negatively charged electrons equal the # of positively charged protons

20. What are valence electrons'? 

electrons in the outermost energy level

21. Define atomic number. Find the atomic numbers of the elements nitrogen, copper, argon, and uranium. 

atomic # is the # of protons in the nucleus of an atom; idenifies a element; 

nitrogen:7

copper:27

argon:18

uranium:92

22.     What group names are given to the elements in Groups 1,2, 3-12, 17, I8'? 

group 1: alkaine metal

group 2: alkaine earth metals

3-12: transition metals

17: haolgens

18: noble gasses

22.     Why are Group 18 elements inert'? 

inert;stable;nontreactive

outer energy is full of valence electrons: 8

Where are the metals, nonmetals, and metalloids found in the periodic table'? 

metals: left of the stair step line

nonmetals: right of the stair step line

metalloid's: elements on the stair step line

25. Define chemical bond. 

26. Distinguish between a compound and a mixture

mixtures dont have chemical bonds, and are just mixed together.

A compound is 2 or more types of elements that have been chemically bound to form a new substance. A mixture is 2 or more atoms of different types that are mixed together without being chemically bound.

Describe the attraction between particles in gases, liquids, and solids. 

liquids-farther apart

solid-closest togetger

gas-furthest apart;plasma

solid: paricles are close togetger and have only enough energy to vibrate in place. have definate volume

liquid: particles have enough energy to move out of arangment and flow past each other have definite volume, and flow to the shape of their container

gas: particles have enough energy to break free of each other and move in all directions have indefinite shape and volume

plasma: free moving ions and electons

28. Why do atoms form compounds'? What makes an atom chemically stable? 

atoms for compounds to become stable, they become stable when there outermost energy level is full of 8 valenece electrons

do this by losing/gaining electrons/stable when 8

29. Define ionic bond, covalent bond, and metallic bond.

ionic bond:the attractive force between oppositely charged ions, which form when electrons are transferred from one atom to another.

covalent bond:a bond formed when atoms share one or more pairs of electrons

metallic bond: a bond formed by the attractive between positively charged metal ions and the electrons around them

30.     What type(s) of elements are present in covalent bonds'? ionic bonds'? metallic bonds? 

COVALENT: NONMETAL & NONMETAL

IONIC BONDS: METAL & NONMETAL

METALLIC BONDS: TWO METALS

   Why can metals conduct electricity'? 

BC valence electrons are free move from atom to atom; the flow of atoms is the flow of electricity

32. Describe the structures and properties of ionic and covalent compounds. 

ionic compounds: 

33. Which types of compounds use prefixes in their names'? 

what is a balanced chemical equation

35.     List 3 signs that a chemical reaction is occurring. 

change in order

change in color

production of a solid

35.     State the law of conservation of mass. 

Name and show models of the 5 types of chemical reactions. 

synthesis: A+B -> AB

decomposition: AB -> A+B

single displacement: A+Bx -> Ax+B

double displacement: Ax+By -> Ay+Bx

combustion: CxHy+O2 -> CO2+H2O

39.     What are coefficients? What are subscripts'? 

coafficients: to the left of a formula and are used to balance equations

Ex. 2HI

subscripts: indicate the # of each atom in a compound

Ex. I2

Name 4 factors that can speed up chemical reactions

increasing temp

increasing surface area

increasing concentraion

increasing pressure (with gasses)

41. What is an enzyme?

An enzyme, is a molecule wither protein or RNA that acts as a catalyst in biochemical reactions.

Give 3 examples of chemical properties.

flammability

ability to rust

reactivity

Define solution, homogeneous mixture, and heterogeneous mixture.

solution: a homogeneous mixture throughout which two or more substances that dissolves in the solvent.

homogeneous: the compounds are evenly distributed, the mixture is same throughout

heterogeneous: substances are not evenly distributed,

44. Define heat of fusion

energy required to change a solid to a liquid

45. Define heat of vaporization

energy required to change a liquid into a gas

Compare the movement of particles in solids, liquids, and gases. 

solid: paricles are close togetger and have only enough energy to vibrate in place. have definate volume

liquid: particles have enough energy to move out of arangment and flow past each other have definite volume, and flow to the shape of their container

gas: particles have enough energy to break free of each other and move in all directions have indefinite shape and volume

plasma: free moving ions and electons

Hetero: vegetables of a saled, sandwich, beach sand, shirts, 

Homo: sugar water, brewed tea or coffee, air

Compare and contrast solutions, suspension, and colloids. 

olutions & colloids have particles that don't settle, whereas particles in a suspension do settle.

group 1: 1

2: 2

13: 3

14:4

15: 5

16: 6

17: 7

18: 8

List 3 properties of metals and 3 properties of nonmetals

metals: hard, shiny,flexible, conductive

nonmetals: gaseous or brittle, dull solids, non conductive

56. How are graphs and tables used by scientists? 

graphs and tables are used by scientists to organize adn present data

57. Define model. 

Model: is a representation of an object or event that can be studied to understand the real object or event

58. Define constant and control

constant: are the things that are kept the same each time one of the trials in the experiment is repeated. For example, constants could include the amount of water used, the brand of effervescent tablet used, the type of water used, and the fact that the water was not stirred. As many outside factors as possible should be keptconstant in an experiment so that the researcher can be sure that any changes that occur do so because of the independent variable.

control: he control is the standard against which the researcher compares the results from each treatment group (level) in theexperiment. the unchanged and not effected during an experiment

61. independent: amount of fertilizer

dependent: growth

62.sample 1

63.. Soil type, sunlight, water, plant type, etc.

65. Give 3 examples of physical changes.

Tearing paper, melting wax, breaking chalk

66.  If the mass of the reactants in a chemical reaction is a total of 35 grams, what will be the total mass of the products in that reaction? 

66. 35 g

67. P = + N = neutral; E = -

An atom contains 12 protons and 13 neutrons. Another contains 12 protons and 15 neutrons. They are___. 

68. Isotopes

70. Sodium nitrate; ammonium sulfate; aluminum hydroxide

71. MgSO4, Ca(OH)2, Al(NO3)3

73. left = reactants; right = products

74. Coefficients are: 1, 1, 1;   1, 5, 3, 4;   1, 6, 3, 2

76. Compound breaks down into simpler substances.

77. (aq), (s), (l), (g)

78. One element replaces a similar element in a compound.

. Endothermic – reaction that absorbs energy; exothermic – reaction that releases energy.

 81. An atom contains 4 protons and 6 neutrons. Another contains 5 protons and 5 neutrons. How do they differ? How are they similar?

83. What were Mendeleev's contributions to the periodic table

83. Organized elements into periodic table by atomic mass, putting similar elements in groups.

84. What charge is acquired when the following atoms form ions: AI, Na, N, F, S, and Ca? 

84. Al 3+, Na+, F-, S2-, Ca2+

86. +1, +2, +3, +4 or +2, -3, -2, -1

87. Give 3 examples of chemical changes.

87. Burning, rusting, neutralizing acid, metal reacting with acid, decomposition, etc.

88. What happens in a chemical reaction?

88. Substances are converted into new substances

89. Define mass number.

89. protons + neutrons

90. What are isotopes?

Atoms with same number of protons but different numbers of neutrons.

. What were Moseley’s contributions to the periodic table?

Organized periodic table by increasing atomic number as well as properties.

93. How do you determine how many valence electrons an element has?

93. By group number.

94. Consider sublimation, melting, freezing, evaporation, and condensation. Which release energy? Which absorb energy?

. Release -  freezing, condensation; Absorb – melting, sublimation, evaporation

95. State Boyle’s law and write the equation that represents it.

As the pressure of a gas increases, its volume decreases if temperature is constant. P1V1 = P2V2

97. What instrument is used to measure mass? temperature? volume?

Mass – balance; temp – thermometer; volume – graduated cylinder, pipet, buret, etc.

99. Describe Rutherford’s gold foil experiment.

Shot alpha particles at gold foil; most went through, a few bounced back or deflected because they hit the nucleus. Rutherford discovered the nucleus

100. Which groups on the periodic table will form negative ions?

100. groups 15 – 17.

101. Which element is found in all organic compounds?

carbon

102. What types of bonds are found in organic compounds?

103. How are groups and periods arranged on the periodic table?

103. Groups are vertical columns.

104. List 3 ways to make a solid solute dissolve more quickly in a solvent.

104. Stir, heat, crush the solid

104. List 3 ways to make a solid solute dissolve more quickly in a solvent.

104. Stir, heat, crush the solid

105. Give two examples each of polar and nonpolar substances

105. Polar – water and alcohol; nonpolar – gasoline and oil

107. Define polar molecule.

Molecule with a positive charge on one end and a negative charge on the other end.

Define saturated solution and unsaturated solution.

What happens in a neutralization reaction?

110. acid + base à salt + water

• 111. Acids taste sour, pH below 7, turn blue litmus red, electrolytes; bases taste bitter, feel slippery, pH above 7, turn red litmus blue, electrolytes.

Define polar molecule and nonpolar molecule.

114. polar – water , vinegar; nonpolar – gasoline, oil

When a change is made to a system in equilibrium, the equilibrium shifts to oppose the change.