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Daily Challenges
FOOD FOR THOUGHT
Once upon a time in a land far away kings used to
use their foot size as a means of determining length.
One king ordered 36 kings feet of expensive royal
fabric from a neighboring country. When the king
received his fabric it was only 27 kings feet. Angry
that he was being cheated, he declared war on his
neighboring country. The fighting lasted for several
years. What do you think caused the fighting?
What could have been done to prevent this war?
AM #2
1. What is the fear of the number 13 called?
2. What are the 6 metric prefixes?
3. What units do we use to measure volume ?
4. How many kiloliters are in 500 liters?
Answers
 Answers:
1. TRISKADEKAPHOBIA
2. KILO; HECTO; DEKA; DECI; CENTI; MILLI
3. Milliliters (ml) for liquids and irregular solids
(displacement factor) OR cm3 if a rectangular
solid
4. .5 kl
AM #3
1. Define mass.
2. What is the formula for Density?
3. What are the units for Density?
4. Define temperature.
Answers
1. The amount of matter in a object.
2. D = M/V
3. For a Regular solid – g/cm3; for a liquid or an
irregular solid – g/ml
4. The amount of ENERGY in an object.
AM #4
1. 6.2 km = ? M
2. The mass of an object is 25g and the volume is
5ml. What is the density?
3. Compare and Contrast accuracy and precision.
4. What is a controlled experiment?
Answers
1. 6200m
2. 5g/ml
3. Accuracy – exactness of your measure and skill
(rounding to nearest .01) Precision – ability to
replicate - following the directions exactly as
they are written every time.
4. A controlled experiment is one where one
variable remains the same (called the control).
This is like a point of reference for the
experiment. Other variables may be changed
(independent variables).
AM # 5
1. Compare a dependent and an independent
variable.
2. Differentiate between a theory to a law.
3. Compare quantitative and qualitative data.
4. 6783.49 cl = ? dkl
Answers
1. An independent variable is what you change in
an experiment. A dependent variable is the
result of changing the independent variable.
2. A theory cannot be concretely proven. A law
states a fact.
3. Quantitative – numerical data; Qualitative –
details (color, condition, etc.)
4. 6.78349dkl
AM #6
1. An object has a density of 1.8 g/ml. Will the
object sink or float?
2. What tools do you need to calculate density?
3. Give an example scenario where accuracy is of
the utmost importance.
ANSWERS
1. Sink (Density greater than 1)
2. For a regular solid: metric ruler/meter stick and
a scale/triple-beam balance; For an irregular
solid: graduated cylinder (or sometimes a
beaker), water, and a scale/triple-beam balance.
3. Answers will vary
AM #7
1. Differentiate between weight and mass.
2. What unit do we use to measure weight and
force?
3. What tools are used for measuring mass (and
weight)?
ANSWERS
1. Mass is the amount of matter in an object.
Weight is the gravitational force that is exerted
on an object.
2. Newton
3. Mass: triple-beam balance/scale and spring
scale; Weight: spring scale/scale
AM # 8
1. Compare mass and inertia
2. Define ductility.
3. What does it mean if a substance is malleable?
4. The temperature of an acid solution is 250C. A
strip of magnesium is added and the
temperature rises 20C each minute for the first 3
minutes. After another 5 minutes the
temperature has risen 2 more degrees. What is
the final temperature?
ANSWERS
1. Mass is a measure of inertia. The more mass an
object has, the more inertia it has.
2. The ability to be pulled into wires. (Copper)
3. The substance can be hammered and rolled into
sheets. (Aluminum)
4. 330C
AM #9
1. How does a chemical change differ from a
chemical property?
2. What are the signs of a chemical change?
3. Generally speaking, is a chemical change
reversible? Why or Why not?
4. Which of the following is a chemical property?
Malleability, Ductility, Conductivity, or Density
ANSWERS
Chemical changes occur when one or more
substances are changed into entirely new
substances with new properties. Chemical
properties determines whether chemical change
will occur.
2. Change in color or odor, production of heat, fizzing
and foaming, sound or light being given off, etc.
3. A chemical change constitutes a change in
composition. It is virtually impossible to revert an
object to its original composition.
4. Conductivity – ability to conduct an electrical charge
1.
AM # 10
1. Compare the 3 states of matter in regard to
placement of particles.
2. How is a plasma classified as a state of matter?
3. Compare Boyle’s Law to Charles’ Law.
4. What happens to a helium balloon when it is
taken outside on a cold winter day? Explain why.
ANSWERS
Solid: particles tightly packed; liquid: particles
loosely packed – enough to where they can slip past
one another; gas: particles are widely dispersed
2. An ionized gas. It only exists on the earth in the
form of lightning. Almost impossible to
harness…Plasma makes up about 99% of the matter
in the universe.
3. Boyle: constant temperature – volume increases as
pressure decreases. Charles: constant pressure –
volume increases and temperature increases
4. Balloon deflates – example of Charles Law (as
temperature decreases, volume decreases)
1.
AM #11
1. Compare elements, mixtures, and
compounds.
2. What are the three classifications
of elements?
3. Give an example of an element, a
mixture, and a compound.
4. Compare a solute to a solvent.
ANSWERS…
1. Element – as simplistic as a substance can be
without losing its properties; Mixture –
substances that are NOT chemically
combined; Compound – substances that ARE
chemically combined
2. Metal, Nonmetal, Metalloid
3. Element: Neon; Mixture: salad; Compound:
Water
4. A solute is dissolved in a solvent.
AM #12
1. What is concentration?
2. How can we change the
solubility rate?
3. Give an example of a colloid
and a suspension.
4. What is the universal solvent?
ANSWERS
1. The ratio of solute to solvent.
2. Can be manipulated by heat.
3. Colloid: jello, milk,
mayonnaise; Suspension:
Italian Salad Dressing,
Homestyle Orange Juice
4. WATER!!!
AM #13
1. Define an atom.
2. Compare an atom, element,
molecule, and a compound.
3. What makes John Dalton
special?
4. What Greek Philosopher came
up with the idea for an atom?
ANSWERS
1. Smallest particle into which an
element/substance can be cut.
2. Atom – smallest particle of an element;
element – pure substance (on periodic
table); molecule – any two chemically
bonded ATOMS; compound – any two or
more chemically bonded ELEMENTS
3. He was the first to develop an atomic theory.
4. Democritus
AM # 14
1. Who’s theory about the atom was called
2.
3.
4.
5.
“plum pudding?”
What is Rutherford credited for?
What unit do we use to measure atomic
mass?
What charges do the subatomic
particles hold?
Where can the subatomic particles be
found inside the atom?
ANSWERS
1. J.J. Thomson
2. The positively charged nucleus
3. Atomic mass unit (amu’s)
4. Proton = +; Neutron = neutral; Electron
=5. Protons and Neutrons – inside the
nucleus; Electrons – in the electron
clouds spinning around the nucleus
AM # 15
1. What does the atomic number tell you?
2. How do you find the number of
neutrons in an atom?
3. How many electrons will the 4 electron
cloud hold?
4. What is an ion?
5. What forces are at work inside an
atom?
ANSWERS
1. How many protons are in the nucleus. Most of
2.
3.
4.
5.
the time it tells you the number of electrons as
well (unless it is an ion).
Take the difference between the atomic number
and the atomic mass (rounded to the nearest
whole number).
32
An electrically charged atom. The number of
protons and electrons are NOT equal. Can be
positive or negative.
Magnetic and Gravitational
AM#16
1. What does the term “periodic” mean?
2. Who was the first scientist to organize
the Periodic Table of Elements?
3. Using your textbook: define “periodic
law.”
4. Using your textbook: What are the only
2 elements that are liquids at room
temperature?
5. What are the 6 metalloids?
ANSWERS…
1. Happening at regular intervals
2. Mendeleev
3. Repeating chemical and physical properties
of elements change periodically (across
periods) with the element’s atomic number
4. Bromine and Mercury
5. Boron (B), Silicon (Si), Germanium (Ge),
Arsenic (As), Antimony (Sb), and Tellurium
(Te)
AM#17
1. What are the vertical columns called on the
2.
3.
4.
5.
periodic table?
What are the horizontal rows called on the
periodic table?
As you move across periods from left to right,
what happens to elements?
What is Group 1 called? What are the common
characteristics of this group?
What is Group 2 called? What are the common
characteristics of this group?
ANSWERS…
1. Groups/Families
2. Periods
3. Elements become less metallic; change
based on a repeating pattern (periodic law).
4. Alkali Metals; highly reactive; one valence
electron; explodes in presence of water
5. Alkaline Earth Metals; reactive; 2 valence
electrons
AM#18
1. Where are the Lanthanides and
2.
3.
4.
5.
Actinides located on the Periodic
Table?
Name 2 elements from these 2 series.
What group is called the Halogens?
Why are the Noble Gases “noble?”
What is the purpose of a valence
electron?
ANSWERS…
1. At the bottom
2. Answers Vary…
3. Group 17
4. The have a full set of valence electrons and
do not feel the need to bond to be complete.
5. They are the electrons that are responsible
for bonding. Commonly called the “hook up”
electrons…
AM#19
1. What happens to chemical bonds
2.
3.
4.
5.
during a chemical reaction?
What are the “magic numbers” in
bonding?
Do the Noble Gases bond?
What kind of elements make up an
ionic, covalent, and metallic bond?
Why would an ion carry a negative
charge?
ANSWERS…
1. The break and the bond again
2. 2 and 8
3. No – they have 8 valence electrons in
their outermost shell
4. Ionic = metal/nonmetal; Covalent =
nonmetal/nonmetal; Metallic =
metal/metal
5. It has gained electrons during the
bonding process
AM#20
1. Why would an ion carry a positive
2.
3.
4.
5.
charge?
Why are ionic compounds neutral?
Give an example of a molecule.
Why can you bend a metal spoon, but
not a wooden spoon?
What is the result of a chemical
reaction?
ANSWERS…
1. It lost electrons during the bonding process.
2.
3.
4.
5.
Therefore the protons outnumber the electrons.
The positive charged metal neutralizes the
negative charged nonmetal. (+2 + -2 = 0)
H2O or O2
Metals bond loosely, therefore they can bend.
Ionic and covalent bonds are more brittle than
metallic bonds.
A chemical bond (or a product).
AM #21
1. What is a precipitate?
2. What are 3 signs of a chemical reaction?
3. How many atoms are in the following equations?
1. H2O
2. C6H12O6
3. 2Al2(SO4)3
4. Label the parts of the following equation.
1. C
+
O2
CO2
5. Balance the following equation.
1. ___H
+ ___ O2
____ H2O
ANSWERS…
A solid particle that forms during a chemical
reaction.
2. Gas formation, precipitate formation, color change,
fizzing, etc…
3. 3,24,34
4. Label the parts of the following equation.
1.
1.
C
+
O2
CO2
5. Balance the following equation.
1. ___H
+ ___ O2
____ H2O
AM #22
1. Explain the Law of Conservation of Mass in
relation to a chemical equation.
2. Give an example of each of the following:
Synthesis
2. Decomposition
3. Single-Displacement Reaction
4. Double-Displacement Reaction
1.
3. What is an endothermic reaction? An
exothermic reaction?
4. What is the Law of Conservation of Energy and
how does it apply to chemical reactions?
ANSWERS…
1.
What ever particles you start with, you also end with.
(Balancing Equations) Matter is NOT created or
destroyed!
Synthesis…Na + Cl = NaCl
2. Decomposition…NaCl = Na + Cl
3. Single-Displacement Reaction
1.
Zn + AgCl
Yields
Ag + ZnCl
4. Double-Displacement Reaction
1.
ZnF + AgCl
Yields
AgF + ZnCl
1.
2. Endo = energy is brought in (on reactant side); Exo =
energy is released (on product side)
3. What ever energy you start with, you finish
with…energy is NOT created or destroyed!
AM #23
1. What kind of energy is required to start a
chemical reaction?
2. What are 5 ways we can manipulate a
3.
4.
5.
6.
Chemical Reaction?
What is an indicator?
Describe an acid.
Describe a base.
How does the pH scale work?
ANSWERS…
1. Activation energy
2. Temperature, concentration, inhibitor,
catalyst, surface area
3. Substance that changes color in the presence
of an acid or base
4. Sour, toxic, corrosive
5. Bitter, slippery, conducts electrical current
6. 1-14 – lower numbers are acids; higher
numbers are bases; 7 is neutral
AM#24
1. What is the formula for speed?
2. Calculate the speed: 50meters and 10seconds
3. What is velocity?
4. Define acceleration.
5. What are the 2 types of acceleration?
6. What do we call continuous acceleration in a
circle?
7. Define force. What unit do we use to measure
force?
ANSWERS
1. Speed = Distance ÷ Time
2. 5m/s
3. Speed in a SPECIFIC direction (45m/s NW)
4. Any change in velocity (speed or direction)
5. Positive and Negative (Deceleration)
6. Centripetal Acceleration
7. A push or pull; the newton (N)
AM#25
1. Describe net force.
2. What happens when forces are traveling in the
3.
4.
5.
6.
same direction? In the opposite direction?
Describe a balanced force. What can balanced
forces NOT do?
Describe an unbalanced force. What can
unbalanced do?
How is friction involved in unbalanced forces?
What 2 factors affect friction?
ANSWERS
1. The combination of all forces acting on an
2.
3.
4.
5.
6.
object.
Same direction = add; Opposite direction =
subtract
An object that has constant velocity or is
completely still; cannot start motion!
An object in motion; can begin or change
motion!
Friction is a factor to increase or decrease
motion/unbalanced force.
Force applies; roughness of the surfaces
AM #26
1. What are the 2 kinds of friction?
2. State one way that friction can be helpful and
3.
4.
5.
6.
one way that friction can be harmful.
What is gravity? What unit do we use to measure
gravity?
What do you have to overcome to lift an object?
What are the 2 parts of the Universal Law of
Gravitation?
Differentiate between weight and mass.
ANSWERS
1. Kinetic and Static
2. Slowing down your car = helpful; friction in a car
3.
4.
5.
6.
engine = harmful
Force of attraction between objects; newtons
Earth’s gravity
Gravitational force increases as mass increases;
gravitational force decreases as distance
increases
Weight is variable; Mass is constant
AM#27
1. 100 grams = ? In Newtons
2. How do we represent gravity numerically?
3. What is the formula for calculating the change
in velocity?
4. Calculate the change in velocity: A penny falls
from a stairwell and travels 7 seconds. What is
it’s velocity as it hits the ground?
5. How does air resistance affect gravity?
6. What is terminal velocity?
ANSWERS
1. 1 newton
2. 9.8 m/s2
3. ΔV = G X T
4. 68.6 m/s
5. Air resistance opposes gravity; it is a type of
friction
6. The point at which air resistance and gravity
reach equilibrium and the object no longer
accelerates.
AM #28
1. Where is the only place an object can be in a true
2.
3.
4.
5.
free fall?
What 2 movements/motions are involved in
projectile motion?
What does Newton’s First Law State? Give an
example.
What is inertia?
How are mass and inertia related?
ANSWERS
1. In orbit (in space)
2. Horizontally then down (vertical)
3. Object in motion stays in motion, object at rest
stays at rest until an unbalanced force acts upon
it; bumper cars
4. Tendency of an object to resist a change in
motion
5. As mass increases, inertia increases…the larger
the object, the more inertia it has…compare
stopping an 18-wheeler to a Prius
AM #29
1. What is Newton’s Second Law of Motion?
2. Give an example of Newton’s 2nd Law.
3. What are the 2 factors involved in Newton’s
4.
5.
6.
7.
Second Law?
What is the formula for acceleration?
What is the formula for calculating force?
What is the acceleration of a 7kg mass if a force
of 68.6N is used to move it toward Earth?
What force is necessary to accelerate a 1,250kg
car at a rate of 40m/s2?
ANSWERS
1. The acceleration of an object depends on the
2.
3.
4.
5.
6.
7.
mass of the object and the force applied.
Compare pushing an empty grocery cart to a full
grocery cart. Which is easier to start and stop.
Mass and Force
A= Force ÷ Mass
F= Mass X Acceleration
9.8 m/s2
50,000N
AM#30
1.
2.
3.
4.
5.
6.
7.
8.
9.
What does Newton’s Third Law state?
Give an example of Newton’s 3rd Law.
Define Momentum.
How does the Law of Conservation of
Momentum work?
Define Work.
What formula do we use to calculate work?
What is the unit we use for work?
What is Power?
How do we calculate Power?
ANSWERS
1.
2.
3.
4.
5.
6.
7.
8.
9.
For every action there is an equal and opposite reaction.
Bouncing a ball
The product of mass and velocity
Momentum is not created or destroyed; it is simply transferred
Transfer of energy where force and object are traveling in the
same direction.
W = Force X Distance
Joules
P = Work ÷ Time
Watt
AM #31
1. What is Power?
2. How do we calculate Power?
3. Define a machine.
4. Is it possible for any machine to have 100%
efficiency? Why or Why not?
5. What are the 3 classes of levers? Give an example
of each.
6. What are the 3 kinds of pulleys? What is the
advantage of the Block and Tackle pulley?
ANSWERS…
1.
2.
3.
4.
5.
6.
See previous AM
See previous AM
Device that makes work easier by manipulating
force
No, because of friction no machine can ever be 100%
efficient.
1st class = see saw; 2nd class = wheelbarrow; 3rd class =
swinging a hammer
Fixed, Movable, and Block and Tackle; Block and
Tackle adds extra wheels so that the weight is
distributed evenly…if there are 4 wheels, each wheel
takes 25% of the weight.
AM #32
1. Give an example of a wheel and axle.
2. Give an example of an incline plane.
3. Give an example of a wedge.
4. Give an example of a screw.
5. What is a compound machine?
6. Define energy.
7. What are the 2 kinds of energy?
8. What is GPE? How do you calculate GPE?
ANSWERS…
1.
2.
3.
4.
5.
6.
7.
8.
Doorknob
Ramp
Knife
Screw
When more than one simple machine are combined.
Ability to do work.
Kinetic and Potential
Gravitational Potential Energy (higher you raise the
object, the more potential energy it has);
GPE = weight X height
AM #33
1. What is mechanical energy?
2. What is thermal energy?
3. Why is chemical energy important?
4. How does electrical energy work?
5. How does sound energy travel? Can sound travel
in space?
6. What is special about light energy?
7. What are the 2 kinds of nuclear energy?
ANSWERS…
1.
2.
3.
4.
5.
6.
7.
Total energy of motion (KE) and position (PE)
All KE due to random movement of particles (heat).
Energy of a compound as atoms rearrange (food).
Energy of moving electrons.
Sound energy travels by vibrating particles. Sound
cannot travel in space since it is a vacuum.
Light can travel through any matter – particles are
not required.
Fission – splitting of the nuclei; Fusion – fusing
(coming together) of nuclei
AM #34
1. What is energy conversion?
2. Describe how the conversion of electrical energy
3.
4.
5.
6.
7.
works?
What can change energy into different forms?
Define friction.
Summarize the Law of Conservation of Energy.
What type of energy does an object have to have
to convert?
Is perpetual motion possible?
ANSWERS…
1.
2.
3.
4.
5.
6.
7.
Change from one form of energy to another.
Light energy and thermal energy can be converted to
electrical energy so that you can turn on a lamp and
the light glows.
Machines
Force that opposes motion.
Energy is NEVER created or destroyed, it is simply
transferred.
Thermal energy (heat)
No, 100% efficiency is NOT possible where friction
exists.
AM #35
Define temperature.
2. What is the boiling point of each scale (C, K, and F)
3. What is the freezing point of each scale (C,K, and F)
4. What is thermal expansion and why is it significant?
5. What is absolute zero? Is absolute zero possible to replicate?
6. What is heat?
7. What is Thermal Conduction? Give an example.
8. Define (thermal) insulators and (thermal) conductors.
9. What is convection? Give an example.
10. What is radiation? Give an example.
11. Define specific heat.
1.
ANSWERS…
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
Measure of average KE of particles.
212OF; 100OC; 273K
32OF; 0OC; -273K
Roads and bridges need extra space to expand
Point where all motion stops; -459OF, -273OC; 0K; it’s NOT possible to replicate
absolute zero
Energy transferred between objects of 2 different temperatures.
Transfer of energy by direct contact; touch a hot pot
Conductors: conduct thermal energy; insulators: do not conduct thermal
energy
Transfer of energy by fluid in a circular patters; convection currents
Transfer of energy by electromagnetic waves; sun on your face (heat you can
feel)
Amount of energy needed to change the temperature of an object by 1OC