Download Midterm Review - Closter Public Schools

Structure and Properties of Matter
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Definition: All matter has ______________________ and ______________________.
Give three examples of matter_______________________________________.
What is not matter?_________________________________________________.
Definition: Mass is a measure of __________________________________________.
When you measure mass you use a ___________________ and express your answer in
________________.
Definition: Weight is a measure of ________________________________________.
When you measure weight, you use a __________________and express your answer in
________________.
Definition: Volume is a measure of ___________________________________________.
When you want to find the volume of a regular solid, you derive it using a formula.
Write the formula here ____________________________. The unit is ______________.
When you want to find the volume of a liquid, you use a tool called a _____________________.
The unit is ____________.
When you want to find the volume of an irregularly shaped solid, use the
_____________________method.
Briefly explain the steps here
______________________________________________________________________________
______________________________________________________________________________
______________________________________________________________________________
Math: What is the volume of a box that has is 12 cm long, 6 cm wide and 4 cm high?
______________________________________________________________________________
Math: If you place a rock into a graduated cylinder containing 50mL of water, and the water
level rises to 57 mL, what is the volume of the rock?
All matter is made of _____________________. They are extremely small.
When two or more atoms bond together, they form a particle called a ____________________.
Atoms and molecules are always moving. In solids, they __________________________. In
liquids, they _____________________________. In gases they ________________________.
Matter is said to be ______________ when it is has only one type of particle.
Matter is said to be ______________when it has more than one type of particle.
A ______________ is a pure substance that contains only a single type of atom.
A ______________ is a pure substance that consists of two or more different types of atoms
bonded together.
A ______________ is a combination of different substances that remain the same individual
substances and can be separated by physical means.
Defintion: The different forms in which matter can exist are called
_______________________________.
This substance has a definite shape and definite volume ____________________.
This substance has a indefinite shape and definite volume___________________.
This substance has neither a definite shape nor volume _____________________.
26. __________________ states that for a fixed volume of a gas at constant temperature, when
pressure increases, volume decreases.
27. __________________states that for a fixed volume of gas at a constant pressure, when
temperature increases, volume increases.
28. Can an oxygen canister ever be half empty? Explain.
______________________________________________________________________________
______________________________________________________________________________
29. Label each graph with the name of the gas law represented.
30. Label each diagram
31. ______________ properties can be observed without changing the identity of the substances.
32. ______________properties describe how a substance can form new substances.
Match each property with its definition.
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________surface tension
________malleability
________flammability
________ductility
________viscosity
a. ability to be formed into a wire
b. difficulty to pour
c. the cohesive force between liquid molecules
d. ability to be pounded into a sheet
e. ability to burn
Identify each property as chemical or physical
38. ______________ reactivity with acid
39. ______________density
40.______________solubility
41.______________flammability
42. ______________color
43._______________odor
44. Density is a very important property of matter. What is the formula for density?
_________________________________________________________________
45. How can density be used to determine if an object will float?
46. How can density be used to identify an unknown piece of matter?
47. A _____________ change is a change in any of the physical properties of a substance, but does
not change the identity of the substance.
48. A ______________change is the change of one substance into another substance.
49. List the four signs that a chemical change has occurred.
______________________________________________________________________________
______________________________________________________________________________
Identify each change as chemical or physical
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____________ burning paper
____________cutting paper
____________iron rusting
____________vinegar and baking soda reacting
____________silver tarnishing
____________slicing butter
____________melting butter
____________baking a cake
____________cooking an egg
____________boiling water
60. ____________________ properties do not depend on the amount of the substance present and
can be very helpful in identifying matter.
61. Mixtures can be separated using their properties. Design a procedure for separating iron filings,
sand, salt and rocks.
63. Label each section of the heating curve above.
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64. What is the melting point of the substance?
65. What is the boiling point of the substance?
Vocabulary
Matter
Chemical property
Mass
Chemical change
Weight
Melting
Volume
Melting point
Atom
Freezing
Molecule
Freezing point
Element
Evaporation
Compound
Sublimation
Mixture
Deposition
States of matter
Boiling
Solid
Boiling point
Liquid
Condensation
Gas
Physical property
Density
Physical change
Math in Science
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What is the volume of a mattress that is 135 cm long, 100 cm wide and 30 cm high?
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A drawing table is 50 cm long, 75 cm wide and 5 cm thick. What is its volume?
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A box of chocolates is 16 cm wide, 30 cm long and 3 cm tall what is the volume of the box?
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A rock is placed in a graduated cylinder with 40 mL of water. The water level rises to 51 mL. What is the
volume of the rock?
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An irregularly shaped object is placed in a graduated cylinder containing 67 mL of water. The water level
rises to 78 mL what is the volume of the rock?
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A bar of copper has a mass of 216g and a volume of 24 cm3. What is the density of copper?
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What is the density of a book that has a mass of 400g and a volume of 600 cm 3?
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The volume of a candy bar is 55 cm3. The mass of the candy bar is 70g. What is the density of the candy
bar?
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A cube has a volume of 36cm3 . If the cube has a mass of 33.2g, what is the density of the cube?
10. Will the cube from problem #9 float on water? Explain.
Interactions of Matter
Many scientists over a long period of time contributed to the development of the atomic theory. Match each
scientist with his contribution.
D= Democritus
DL= Dalton
T= Thomson
R= Rutherford
B= Bohr
S&H= Schrödinger and Heisenberg
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_________ Performed the cathode-ray tube experiment which led to the discovery of electrons.
_________ First proposed the idea of the atom- the “uncuttable” particle.
_________Performed the gold foil experiment and discovered the nucleus
_________Said that electrons do not move in definite paths, but are found in clouds.
_________Said that electrons move in definite paths and can jump from path to path.
_________He published the first atomic theory that proposed that atoms cannot be created or destroyed.
Label the diagram of the atom.
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The atomic number tells you the ___________________________________________________.
The atomic mass number tells you the ______________________________________________.
Explain how you can use atomic number and atomic mass number to determine the number of neutrons
in an atom.
10. Atoms are always electrically neutral; therefore, the number of protons and electrons is always ________.
11. __________________ are atoms of the same element that have a different number of neutrons.
Fill in the chart
Element
Symbol
C
Cl
Ne
Atomic
Number
6
8
17
Mass Number
Number of
Protons
Number of
Neutrons
Number of
Electrons
Isotope
notation
12
O-16
18
20
12. The ________________________ is the weighted average of all of the naturally occurring isotopes of a
given element.
13. _________________________ organized the first periodic table.
14. He organized the periodic table by ____________________; it was later reorganized by
______________________.
15. He left gaps in his table where no elements existed that fit the pattern. He predicted that these elements
would _______________________.
16. A ____________________ is a vertical column on the periodic table.
17. A ____________________ is a horizontal row on the periodic table.
18. The periodic table can be divided into three distinct regions: metals, non-metals, and metalloids. List the
properties of each here. Metals ________________________________________________
Nonmetals______________________________________ Metalloids ______________________________
19. Elements can be organized into families that have similar properties. Record some of the properties
associated with each family here.
Alkali metals
Alkaline-Earth Metals
Transition Metals
Halogens
Nobel Gases
Lanthanide & Actinide series
Hydrogen
20. Some elements are radioactive and undergo radioactive decay. A _____________________ is the amount
of time it takes for one-half of a particular sample of an isotope to decay.
21. How do the properties of a compound compare to the properties of the elements that formed
them?_____________________________________________________________________________
22. A ________________________ uses chemical symbols and subscripts to represent the atoms of elements
and their ratios in an compound.
Complete the chart
Formula
CH4
H2O
H2O2
Elements
Ratio
Total atoms
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An ________________________ is the force of attraction between positive and negatively charged ions.
_________________ form positive ions when they _______________ electrons.
_________________form negative ions when they ________________ electrons.
An ion with a +2 charge has ______________ 2 electrons.
A _____________________ is the force of attraction between atoms that are sharing a pair of electrons.
A _____________________ is a covalent bond in which the pair of electrons is shared unequally.
Ionic compounds have certain properties. List three here __________________________________
Covalent compounds have certain properties. List three here________________________________
Metallic compounds have certain properties. List three here ________________________________
Write the formula for dinitrogen trioxide.__________________________
Write the formula for lithium oxide._______________________________
A ________________________ produces new substances by changing the way in which atoms are
arranged.
35. _________________ are the starting materials in a chemical reaction.
36. _________________ are the ending materials in a chemical reaction.
Classify the following chemical reactions.
_____________________ Na + Cl2  NaCl
_____________________Zn + HCl  ZnCl2+ H2
_____________________H2CO2 H2O + CO2
_____________________NaCL + AgF  NaF + AgCl
List four factors that affect the rate of reaction
______________________________________________________________________________________
______________________________________________________________________________________
42. The ____________________________________ states that matter cannot or created or destroyed in an
ordinary chemical reaction.
43. Balance the following chemical reactions.
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H2 + O2  H2O
F2 + KCl  KF + Cl2
HCl + Na2S  H2S + NaCl
Al + CL2  AlCl3
44. A reaction in which energy is released is called __________________________________.
45. A reaction in which energy is absorbed is called _________________________________.
For each graph, label reactants, products, energy lost or gained, and activation energy.
46. Which graphs represent exothermic reactions?___________________________
47. Which graphs represent endothermic reactions?__________________________
Vocabulary
Proton
metal
precipitate
Neutron
nonmetal
catalyst
Nucleus
metalloid
inhibitor
Electron
radioactivity
chemical reaction
Atomic number
half-life
reactant
Atomic mass number
chemical formula
product
Isotope
subscript
coefficient
Atomic mass
ionic bond
law of conservation of mass
Periodic table
covalent bond
bond energy
group
molecule
endothermic reaction
period
polar covalent bond
exothermic reaction
reactive
metallic bond