Download Semester 1 Exam Review

Semester 1 Exam Review
Comprehensive Science 3
Chapter 8
#31-32
Chemical Compounds
#31 – Compare and contrast acids
and bases (p.216-219)
• Acids
– Any compound that increases the number of
hydronium ions when dissolved in water
– Examples: vinegar, acid rain, soda, lemons
• Bases
– Any compound that increases the number of
hydroxide ions when dissolved in water
– Examples: baking soda, ammonia, soap,
antacids
#32 – How would you classify a substance with a
pH of 7, below a 7, and above a 7? (p.223)
• pH – a value that is used to express the
acidity or basicity of a system
• pH of 7 = neutral
• pH below 7 = acidic
• pH above 7 = basic
Chapter 16
#42-46
Stars, Galaxies, and the Universe
#42 – What makes up the
composition of a star? (p. 465)
• A star is made up of different elements in
the form of gases
#43 – Define apparent and
absolute magnitude (p.468)
• Apparent magnitude
– the brightness of a star as seen from Earth
• Absolute magnitude
– the actual brightness of a star
#44 – Define light-year (p.469)
• The distance that light travels in one year
(about 9.46 trillion km)
#45 – List the life cycle of stars from
the beginning to the end (p.472-473)
1. A star enters the first stage of its life
cycle as a ball of gas and dust
2. After a star forms, it enters the second
and longest stage of its life cycle, known
as the main sequence
3. Red giants
4. Red supergiants
5. White dwarfs – can shine for billions of
years before they cool completely
Hertzsprung-Russell Diagram
(p.474-475)
#46 – Define galaxy (p.478)
• Galaxy
– A large group of stars, dust, and gas held
together by gravity
• Distant vs. early galaxies
– Looking at distant galaxies helps scientists
know what early galaxies looked like
– Gives scientists an idea of how galaxies
change over time
Chapter 17
#47-50
A Family of Planets
#47 – Draw a model of the solar
system (p.496-497)
#48 – Define satellite (p.512)
• A natural or artificial body that revolves
around a planet
– Moons are natural satellites
#49 – Where do comets come
from? (p.520-521)
• Comets are formed in the cold, outer solar
system
#50 – Compare and contrast asteroids,
meteroids, and comets (p.520-523)
• Comets
– A small body of ice, rock, and comic dust that follows
an elliptical orbit around the sun and that gives off gas
and dust in the form of a tail as it passes close to the
sun
• Asteroids
– Small rocks bodies that orbit the sun
• Meteroids
– Small rock bodies that travel through space (similar to
but smaller than asteroids; most are probably pieces
of asteroids)
COMET
METEOR SHOWER
ASTEROIDS
Chapter 18
#33-35
Cells, Tissues, and Organs
#33 – List the levels of structural organization in
multicellular organisms (p.544)
1.
2.
3.
4.
5.
Cells
Tissues
Organs
Organ Systems
Organisms
#34 – Explain the role of mitosis at
the cellular level (p.547)
• Mitosis
– The process of cell division that results in two
new nuclei, each of which has the same
number of chromosomes
#35 – Why are new cells needed? (p.546)
• Cells grow and divide to make more cells
– Cell division allows organisms to grow, repair
damaged tissues, and reproduce
Other Information
• The Human Organism (p.557)
– Some behaviors are a response to stimuli
from the environment
– Your organ systems allow your body to
respond to that stimuli
• Example: You may be scared if you saw an
accident on the interstate
– Your nervous system would cause changes in your body
by making your heart pump blood faster
Chapter 19
#36-41
Heredity
#36 – Define heredity (p. 568)
• Heredity
– The passing of genetic traits from parents to
offspring
#37 – Explain how Punnett squares
are used in science. (p.575)
• Punnett squares
– Used to predict all the
possible combinations
of offspring from
particular parents
#38 – Compare and contrast dominance and
recessive traits. (p.574)
• Dominance
– Occurs when alleles mask the expressions of
other alleles (ex. Pp or PP)
• Recessive
– Describes an allele that will be masked,
unless the organism is homozygous for the
trait (ex. pp)
#39 – Define incomplete
dominance (p.578)
• Incomplete dominance
– Sometimes one trait is not completely
dominant over another; both alleles have
some degree of influence
#40 – Look at the snapdragon cross on
page 578 – Why were pink snapdragons
produced instead of red snapdragons?
Due to incomplete dominance.
#41 – Which types of cells are
made during meiosis? (p.582)
• Meiosis
– A process that produces sex cells with half the
usual number of chromosomes (23)
Chapter 1
#1-6
The Nature of Science
#1 – List the steps of the scientific
method (p.12-18)
#1
1.
2.
3.
4.
5.
6.
7.
Ask a question
Form a hypothesis
Test your hypothesis
Make observations
Analyze the results
Draw conclusions
Communicate results
#2 – Define hypothesis (p.15)
• Hypothesis
– An idea or explanation that is based on
observations and that can be tested
#3 – Explain the information that is
given in a good hypothesis. (p.15)
• A good hypothesis is one that can be
TESTED
#4 – Explain how changing a variable in an
experiment may alter the affects of the
experiment. (p.16)
• Changing a variable may change one or
more parts of the experiment, therefore,
changing the outcome of the experiment
#5 – Calculate the density of an object with a mass
of 20kg and a volume of 10mL. (p.23)
• Density = Mass/Volume
– 20kg/10mL = 2 kg/mL
– 20,000g/10mL = 2,000 g/mL
#6 – Calculate the volume of an object with a
length of 10cm, a width of 5cm, and a height of
2cm. (p.23)
• Volume = Length x Width x Height
– 10cm x 5cm x 2cm = 100 cm3
Chapter 2
#7-8
Science, Technology, and Society
#7 – Define technology (p.42)
• Technology
– The application of science for practical purposes; the
use of tools, machines, materials, and processes to
meet human needs
• Who makes technology?
– Has been made by many kinds of people living in
various cultures at different times
– Every human culture has had its own technology
– No matter where technology starts, it will eventually
becomes available to people everywhere
#8 – List three ways that scientists use
computers and technology. (p.43-45)
• MP3 files, mathematical models, collecting
and sorting data, lasers
Chapter 3
#9-14
Properties and States of Matter
#9 – Define matter (p.76)
• Matter
– Anything that has mass and takes up space
#10 – Define atom (p.76)
• Atom
– The building blocks of matter
– The smallest unit of an element
#11 – Define the states of matter (p.90-93)
• Properties of Solids
• Particles are tightly
packed in a regular
pattern
• Particles don’t move
around easily;
cannot move past
each other
• Retain their shape
#11 – Define the states of matter (p.90-93)
• Properties of Liquids
• Particles are close
together with no
regular pattern
• Particles flow and can
easily move past
each other
• Assume the shape of
their container
#11 – Define the states of matter (p.90-93)
• Properties of Gases
• Particles are spread
out with no pattern
• Particles move freely
at high speed
• Assume the shape of
their container
Changes of State
(boiling)
Energy is
added
Energy is
removed
#12 – Give an example of a chemical
and physical property (p.80-81)
• Physical Property
– Characteristic of matter that can be observed or
measured without the matter going through a
chemical change, or a change in identity
– Examples: shape, mass, odor, texture
• Chemical Property
– Property of matter that describes a substance’s ability
to participate in chemical reactions
– New substances are created
– Examples: reactivity, flammability
#13 – Define the law of
conservation of mass (p.84)
• Law of conservation of mass
– States that mass is not created or destroyed
in ordinary chemical and physical changes
#14 – Give an example of a physical change
and a chemical change (p.85-87)
• Physical change
– Any change in which the physical properties of a
substance change but the substance’s identity does
not
– Examples: salt dissolving in water, water freezing,
water melting, glass breaking
• Chemical change
– When a change occurs and new substances are
formed with identities and properties different from the
original matter
– Examples: paper burning, baking soda mixed with
vinegar, photosynthesis, food digesting
Chapter 4
#15-17
Atoms
#15 – List the particles of an atom
(p.113-114)
Inside the Nucleus
A. Protons
•
Positive charge (+)
B. Neutrons
•
No charge (neutral)
Outside the Nucleus
A. Electrons
•
•
Negative charge (-)
Orbit the nucleus in electron clouds
#16 – Describe the relative size
and parts of a nucleus (p.113)
• Inside the nucleus
– Protons and neutrons
• Outside the nucleus
– Electrons (in electron clouds)
#17 – Describe the role of the
electrons in an atom (p.118)
• Electrons are a very small part of an
atom’s mass
• Form the outer layer of the atom
– Important to the atom’s interactions with its
environment
– Atoms can gain or lose electrons by forming
bonds with other atoms
Isotopes (p.115)
• Isotope – atoms of the same element that
have the same number of protons (same
atomic #) but different numbers of
neutrons (different atomic mass)
– Each element has a limited number of
isotopes found in nature
– Example: Carbon-12 (atomic mass = 12;
atomic number = 6)
• Atomic Mass – Atomic Number = 12 – 6 = 6
neutrons
Chapter 5
#18-20
The Periodic Table
#18 – Define the periodic law (p.131)
• States that the repeating chemical and
physical properties of elements change
periodically with the atomic numbers of the
elements
#19 – What information is given in each
square of the periodic table? (p.132)
Atomic Number
Element Symbol
Element Name
Atomic Mass
protons
electrons
protons
neutrons
#20 – Why are elements grouped together
on the periodic table? (p.131&138)
• Periods
– horizontal row of elements (from left to right)
• Groups
– vertical column of elements (from top to bottom)
– Also called a family
– Each group has the same number of valence
electrons and similar properties
• Elements classified as metals, nonmetals, and
metalloids
Chapter 6
#21-24
Chemical Bonding
#21 – Define chemical bonding (p.158)
• What is chemical
bonding?
• The joining of atoms to
form new substances
• What is a chemical
bond?
• An interaction that
holds two atoms
together
• What happens when
chemical bonds form?
• Electrons are shared,
gained, or lost
#22 – Define valence electrons (p.159)
• An electron in the outermost energy level
of an atom
#23 – What role do valence electrons play in
whether an atom bonds to another atom or
not? (p.160-161)
• The number of valence electrons
determines whether or not an atom will
bond
– 8 valence electrons in the outer shell is a
complete set
– Atoms want 8 valence electrons to be happy!
• To achieve this, atoms will gain, lose, or share
electrons
#24 – What are the role of the electrons in ionic
bonds, covalent bonds, and metallic bonds?
(p.162, 166, 169)
• Ionic Bonding
– A bond that forms when valence electrons are
transferred from one atom to another atom
– Metal atoms lose one or more valence electron and
nonmetal atoms gain electrons
• Covalent Bonding
– A bond formed when atoms share one or more pairs
of valence electrons
– Occurs between nonmetals
• Metallic Bonding
– A bond formed by the attraction between positively
charged metal ions and the electrons in the metal
– Occurs between metals
Chapter 7
#25-30
Chemical Reactions
#25 – Define chemical reaction (p.182)
• A process in which one or more
substances change to make one or more
new substances
– Chemical and physical properties of new
substance are different from the original
substances
#26 – List two signs of a chemical reaction (p.183)
• Signs of Chemical
Reactions
•
•
•
•
Gas Formation
Energy Change
Color Change
Solid Formation
– Precipitate: a solid
that is produced as a
result of a chemical
reaction in solution
#27 – What happens to the bonds of
substances during chemical reactions? (p.184)
• How do new substances form in a
chemical reaction?
– First, the chemical bonds in the starting
substances must break
– Then, the atoms rearrange
– Finally, new bonds form to make the new
substances
#28 – Compare and contrast endothermic and
exothermic reactions (p.196-197)
• Exothermic Reactions
– A chemical reaction in which energy (heat) is
released
– Energy released is written as a product
• X+X
X + energy
• Endothermic Reactions
– A chemical reaction in which energy is taken
in
– Energy taken in is written as a reactant
• X + energy
X+X
#29 – Define the law of
conservation of energy (p.197)
• Law of conservation of energy
– Energy cannot be created or destroyed, but
can be changed or transformed from one form
to another
– Energy in = energy out
#30 – Explain how the factors affecting the rates of
reactions alter the chemical reaction (p.199-201)
• Temperature
– Higher temperatures = faster rate of reaction
• Concentration
– Higher concentration = faster rate of reaction
• Surface Area
– Increased surface area of a solid = faster rate of
reaction
• Inhibitors
– Substance that slows down or stops a chemical
reaction
• Catalysts
– Substance that speeds up a reaction without being
permanently changed