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physical science honors mid-term
mid-term
95
Science
9th Grade
01/12/2011

Additional Science Flashcards

 


 

Cards

Term

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

Definition

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

Term

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

Definition

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

Term

3. Distinguish between a hypothesis and a theory. 

Definition

hypothesis: testable statement/question/educated guess

 

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

Term

4. Describe the steps in the scientific method. 

Definition

series of logical steps to solve problems:

purpose/question

research

hypothesis

experiment

analysis data

draw your conclusion

 

poster on wall

Term
5. Name the SI units for temperature, mass, length, and time
Definition

temp: kelvin

mass: kilogram

length:meter

time:second

Term

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


 

35,000 mg  = ­­­­__ hg

Definition

155cm

 

545ml

 

.35hg

Term
Convert the following: 454 g = __ kg;    1.997 dg = ___dag
Definition

.454kg

 

.01997dg

Term
convert 325000000m; 0.0000024s
Definition

3.25x10^8m

 

 

2.4x10^negative 6s

Term

 

9. Define element and compound. 

 

Definition

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

 

compoundA 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.

Term

Name and                   describe the 4 states of matter. 

 

Definition

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

Term
II. The kinetic theory states   
Definition

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

Term

 

 

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

 

Definition

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: 

Condensation is the process by which matter transitions from a gas (or vapor) phase into a liquid phase.



melting: thaw: the process whereby heat changes something from a solid to a liquid;


sublimation: Sublimation is the transition of a substance from the solid phase to the gas phase without passing through an intermediate liquid phase


freezing: reezing or solidification is a phase change in which a liquid turns into a solid when its temperature is lowered below its freezing point. The reverse process is melting.

 

Term

Give 3 examples of physical properties. 

Definition

color

shape

density

melting point

Term

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

Definition

line graph: shows changes over time

 

pie graph: shows parts of a whole

 

bar graph: used to compare things in different grorps

Term

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

Definition

independent: x

 

dependent: y

Term

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

Definition

density= m/v

 

119/14

 

8.5=d

Term

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

Definition

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

 

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

Term

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

Definition

protons & neutrons

 

nucleus has a positvie charge

 

electron cloud has an negative charge

Term

19. Why do atoms have no electric charge'? 

Definition

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

Term

20. What are valence electrons'? 

Definition

electrons in the outermost energy level

Term

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

Definition

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

 

nitrogen:7

copper:27

argon:18

uranium:92

Term

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

Definition

group 1: alkaine metal

 

group 2: alkaine earth metals

 

3-12: transition metals

 

17: haolgens

 

18: noble gasses

Term

22.     Why are Group 18 elements inert'? 

Definition

inert;stable;nontreactive

 

outer energy is full of valence electrons: 8

Term

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

Definition

metals: left of the stair step line

nonmetals: right of the stair step line

metalloid's: elements on the stair step line

Term

25. Define chemical bond. 

Definition
chemical bond: the attractive force that holds ions or atoms together
Term

26. Distinguish between a compound and a mixture

Definition

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.


Term

 

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

 

Definition

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

Term

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

Definition

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

Term

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

 

Definition

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

Term

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

Definition

COVALENT: NONMETAL & NONMETAL

 

IONIC BONDS: METAL & NONMETAL

 

METALLIC BONDS: TWO METALS

Term

   Why can metals conduct electricity'? 

Definition

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

Term

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

Definition

ionic compounds: 

Term

 

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

 

Definition
covalent
Term

 

 

what is a balanced chemical equation

Definition
chemical equations are balanced when there are the same # of each type of atom on both sides of the arrow
Term

 

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

 

Definition

change in order

change in color

production of a solid

 

Term

 

35.     State the law of conservation of mass. 

 

Definition
mass can not be created or destroyed 
Term

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

Definition

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

Term

 

39.     What are coefficients? What are subscripts'? 

 

Definition

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

Term

Name 4 factors that can speed up chemical reactions

Definition

increasing temp

increasing surface area

increasing concentraion

increasing pressure (with gasses)

 

Term

41. What is an enzyme?

Definition

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

 

 

Term

Give 3 examples of chemical properties.

 

Definition

flammability

ability to rust

reactivity

 

Term

Define solution, homogeneous mixture, and heterogeneous mixture.

Definition

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,

Term

44. Define heat of fusion

Definition

energy required to change a solid to a liquid

Term

45. Define heat of vaporization

Definition

energy required to change a liquid into a gas

Term

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

Definition

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

Term
give 2 examples of homogeneous mixtures and heterogeneous mixtures
Definition

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

 

Homo: sugar water, brewed tea or coffee, air

Term

Compare and contrast solutions, suspension, and colloids. 

Definition

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

Term
how many electrons are in the outer energy level of elements in groups 1,2,13,14,15,16,17,&18
Definition

group 1: 1

2: 2

13: 3

14:4

15: 5

16: 6

17: 7

18: 8

Term

List 3 properties of metals and 3 properties of nonmetals

Definition

metals: hard, shiny,flexible, conductive

 

nonmetals: gaseous or brittle, dull solids, non conductive

Term

56. How are graphs and tables used by scientists? 

Definition

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

Term

57. Define model. 

Definition

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

Term

58. Define constant and control

Definition

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

 


Term
Question on Paper 61
Definition

61. independent: amount of fertilizer

dependent: growth

 

62.sample 1

 

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

 

Term
What makes the elements in Groups 1 and 2 very reactive?
Definition
Only need to lose 1 or 2 electrons to become stable
Term

65. Give 3 examples of physical changes.

Definition

Tearing paper, melting wax, breaking chalk

Term

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? 

Definition

66. 35 g

Term
What are the charges on protons, neutrons, and electrons? 
Definition

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

Term

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

Definition

68. Isotopes

Term

70. Name the following compounds: NaNO3, (NH4)2SO4,  Al (OH)3.

 

Definition

70. Sodium nitrate; ammonium sulfate; aluminum hydroxide

Term
Write formulas for the following compounds: magnesium sulfate, calcium hydroxide, aluminum nitrate
Definition

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

Term
what is adjusted to balance an equation 
Definition
2. Coefficients
Term
what are substances to the right and left of the arrow in a chemical equation called
Definition

 

73. left = reactants; right = products

 

Term
Definition

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

Term
what happens in a decomposition reaction
Definition

 

76. Compound breaks down into simpler substances.

 

Term
in a chemical equation, what are the symbols that mean dissolved in water, solid,liquid, and gas.
Definition

 

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

 

Term
what happens in a single displacement reaction
Definition

 

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

 

Term
define endothermic and exothermic
Definition

 

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

 

Term

 

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

 

Definition
Different elements with the same mass number.
Term

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

Definition

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

Term

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

Definition

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

Term
86. What charges do the elements in Groups 1, 2, 13, 14, 15
Definition

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

Term

87. Give 3 examples of chemical changes.

Definition

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

Term

88. What happens in a chemical reaction?

Definition

88. Substances are converted into new substances

Term

 

89. Define mass number.

Definition

89. protons + neutrons

Term

90. What are isotopes?

Definition

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

Term

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

Definition

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

Term

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

Definition

93. By group number.

Term

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

Definition

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

Term

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

Definition

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

Term

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

Definition

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

Term

 

99. Describe Rutherford’s gold foil experiment.

Definition

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

Term

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

Definition

100. groups 15 – 17.

Term

101. Which element is found in all organic compounds?

Definition

carbon

Term

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

Definition
covalent
Term

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

Definition

103. Groups are vertical columns.

Term

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

Definition

104. Stir, heat, crush the solid

Term

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

Definition

104. Stir, heat, crush the solid

Term

105. Give two examples each of polar and nonpolar substances

Definition

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

Term

107. Define polar molecule.

Definition

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

Term

Define saturated solution and unsaturated solution.

Definition
Saturated solution contains all the solute that can dissolve at a given temperature. Unsaturated solution contains less solute than that amount
Term

What happens in a neutralization reaction?

Definition

110. acid + base à salt + water

Term
Name 3 properties of acids and 3 properties of bases
Definition

  • 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.

Term

Define polar molecule and nonpolar molecule.

 

Definition
Polar molecules have one end that is positive and one end that is negative. Nonpolar molecules have a uniform charge over the entire molecule
Term
. Which of the following are polar?    water, vinegar, oil, gasoline
Definition

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

Term
State Le Chatlier’s Principle.
Definition

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

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