Download standard 1 - Taylorsville-Paxton

Standard 1, objective 1
Chemistry Assessment
a1. What evidence supports the assumption that matter in the universe has a common origin?
a.
b.
c.
d.
analysis of radiation produced by stars
actual testing of matter collected in stars
an educated guess
a mathematical model based on gravity
a2. How does the direction of moving objects in the universe support the common origin of
matter?
a.
b.
c.
d.
objects in space are moving at the speed of light
objects in space are traveling toward one another
objects in space are moving the same speed
objects in space are traveling away from one another
a3. What does analysis of radioactive materials indicate about the origin of matter in the
universe?
a.
b.
c.
d.
it cannot be dated accurately
it was made all at once in many locations
it was all made within the same time period
it shows that stars are constantly making new matter
a4. Radiation from the big bang was discovered accidentally by two scientists looking into
space for something else. Where did they find the cosmic background radiation?
a.
b.
c.
d.
throughout the universe
originating on Earth
coming from exploding stars
near the Sun
a5. What technology is used to observe red shifts of galaxies?
a.
b.
c.
d.
Radio receivers
Spectroscope
Microscope
Satellite
Use the following information to answer the next two questions.
A Belgian priest, Georges Lamaître, was the first to develop a “big bang” theory. In 1927, after
studying red shifts of galaxies, he proposed that the universe began with an immense infusion
of pure energy into space.
Later, Edwin Hubble discovered that the speed of a galaxy moving away from Earth
was proportional to its distance. This relation was predicted by Lamaître’s theory. V.M.
Slipher studied faint, cloud like objects in the sky. He noted that most of the objects had red
shifts and that the fainter the object, the larger the red shift. Then, in 1964, Arno Penzias and
Robert Wilson discovered the cosmic background radiation, which was also predicted by
Lamaître's theory.
a6. Why wasn’t the “big bang” theory accepted by the scientific community when it was first
proposed in 1927?
a. Lamaître did not have enough evidence to support his theory in 1927
b. Historically religious people have not had sound scientific ideas, so his idea was
ignored
c. The government did not like the idea that the universe is continually expanding
d. Scientific evidence from other sources showed blue shifts of most galaxies
b7. What does the information above show about scientific theories?
a. Scientific theories are very field-specific and different studies are not interrelated
b. Scientific theories are cumulative results from many different scientists
c. Due to all this evidence, the Big Bang should be considered a fact, not a theory
d. Lamaître should be given the credit for the Big Bang theory
b8. Which of the following statements about matter in the universe and on Earth is the most
correct? Matter on Earth and in the universe is composed of:
a.
b.
c.
d.
different sub-atomic particles and different elements
some of the same elements, but Earth has more different types
the same elements with the same structure
unknown types of matter
b9. Where have scientists found new elements in the universe?
a.
b.
c.
d.
the outer planets
the nearest galaxy
the closest star
laboratories on Earth
Use this graph to answer the next three questions:
c10. What are the most abundant elements in the universe?
a.
b.
c.
d.
heavy elements, over 60 in atomic number
mid-weight elements, between 20 and 40 in atomic number
light element, between 8 and 20 in atomic number
very light elements, between 1-4 in atomic number
c11. Atoms with large atomic numbers are larger atoms. What general rule seems to be true
about abundance and atom size?
a.
b.
c.
d.
small atoms are least abundant.
the larger the atom, the less abundant it is.
the larger the atom, the more abundant it is.
atom size and abundance do not appear related.
d12. What inference is made from this data about the big bang and elements? The first
elements formed were
a.
b.
c.
d.
small and have been forming larger atoms ever since.
small and large elements were formed during a second explosion.
large and have broken down into smaller and smaller atoms ever since.
large and combined to form even larger elements with small particles leftover
c13. Which graph correctly shows the abundance of elements in the universe?
a.
b.
c.
d.
c14. People have proposed to travel to other planets to mine for elements when we run out of
them on Earth. How likely is it that other planets would have what we need?
a.
b.
c.
d.
Every planet has what we might need.
It is very unlikely other planets would have what we need.
Some planets could have elements we might need.
Space travel is not possible to other planets.
d15. Which of the following statements about the distribution of heavy elements on Earth and
the universe is most correct?
a.
b.
c.
d.
About the same amount of heavy elements exist on Earth and the universe
There is a greater percentage of heavy elements on Earth than the universe
There is a greater percentage of heavy elements in the universe than on Earth
Heavy elements are found in stars, lighter elements are found in planets.
d16. What relationship exists between atom size and abundance in the universe?
a.
b.
c.
d.
the smallest atoms are rare
largest atoms are most abundant
the large atoms are not found with small ones
smallest atoms are most abundant
Chemistry
Standard 1, Objective 2
a1. How did the early ideas about atoms Democritus and Aristotle discussed differ from the
work of scientists that came later?
a.
b.
c.
d.
They did not use experiments to test their ideas.
They correctly measured the size and shape of atoms.
They worked in groups with others.
They used a variety of technology to aid their research.
a2. Rutherford used an experiment that showed how particles pass through a single layer of
gold atoms in gold foil. Occasionally, one of the particles bounced back off the gold foil but
most went through. What did Rutherford prove?
a.
b.
c.
d.
gold atoms are larger than many other atoms..
gold atoms have 79 protons and 79 electrons.
gold atoms have a small positively charged nucleus.
gold atoms have electrons embedded in a “plum pudding” around the nucleus.
a3. Bohr proposed that electrons occur it orbits which have energy levels. How does the
quantum mechanical model predict where the electrons will be?
a.
b.
c.
d.
creating known shells
by guessing
using probabilities
looking as far from the nucleus as possible.
a4. Which of the following is modern technology used to study the nature of the atom?
a.
b.
c.
d.
super colliders
telescopes in space
light microscopes
electric generators
b5. Why must models be made to help study atoms?
a.
b.
c.
d.
they cannot be captured.
they are difficult to find
they do not have parts.
they are too small to see
b6. Which of the following is a way the picture on
the right can correctly describe an atom? The model:
a.
b.
c.
d.
is the right size
has moving electrons
is three dimensional
shows the charges on atomic particles
b7. Which of the following most accurately models the nature of atoms and their movement?
a.
b.
c.
d.
a frozen bag of peas
a pan of water
shaking a box of marbles
pouring a liquid from container to another
c8. How is a proton different from a neutron?
a.
b.
c.
d.
a proton is negatively charged, a neutron is neutral.
a proton is positively charged, a neutron is neutral.
a proton has a mass of 1, a neutron is much less.
a proton is found in the nucleus, a neutron is not.
c9. Which is the most accurate model comparing an electron compared to a proton?
a.
b.
c.
d.
like a mosquito to a house.
like a person in a truck
like a tree growing in Earth.
like a page torn from a book.
c10. Where would you expect to find protons?
a.
b.
c.
d.
in the outer shells
in the “d” orbital
in the nucleus
attached to the electrons
c11. If an atom were the size of a football stadium, how big would the nucleus be at the center?
As large as:
a.
b.
c.
d.
a pea
a basketball
a house
a grocery store
c12. Which statement best describes the position and charge of an electron?
a.
b.
c.
d.
Located in the nucleus and has a negative charge
Located in the nucleus and has a positive charge
Located outside the nucleus and has a negative charge
Located outside the nucleus and has a positive charge
c13. How does the relative size of an electron compare to a proton?
a.
b.
c.
d.
Protons and electrons are about the same size
A proton is nearly 2,000 times more massive than an electron
An electron is nearly 2,000 times more massive than a proton
Electrons have energy, not mass
d14. What does the proton number indicate about the atom?
a.
b.
c.
d.
the mass of the atom
the atomic number of the atom
the number of neutrons in the atom
the number of electron orbitals
d15. The atomic number of carbon is 6. What information does that provide?
a.
b.
c.
d.
carbon has 6 neutrons.
carbon is a solid, black substance.
carbon has 6 electrons and 6 protons
carbon can bond with many other substances.
d16. A radioactive atom loses protons from its nucleus during radioactive decay. What is the
result?
a.
b.
c.
d.
it becomes a different element
it gains atomic weight
it will react with more kinds of elements
it has more electrons
d17. Which of the following would be most useful in determining the identity of an element?
a.
b.
c.
d.
The number of electrons
The number of protons
The number of neutrons
The shape of electron orbits
d18. How many protons are in a Sulfur atom?
a.
b.
c.
d.
8
16
32
6.02 x 1023
e19. Which of the following is the best an analogy for a mole?
a.
b.
c.
d.
describing eggs by the dozen.
the sun holding the planets in orbit.
measuring NaCl by the gram.
opening surprise packages.
e20. Carbon has a mass of 12. How many atoms of carbon are in a 12 gram sample?
a.
b.
c.
d.
an unknown quantity
12 million
12 billion
6.02 x 1023
e21. What is the molar mass of H2O?
a.
b.
c.
d.
6g
16 g
18 g
24 g
e22. How many atoms are in one mole of Iron?
a.
b.
c.
d.
8
16
6.626 x 10-34
6.02 x 1023
e23. What is the mass of one mole of Oxygen gas (O2)?
a. 8 grams
b. 16 grams
c. 32 grams
d. 6.02 x 1023 grams
Chemistry
Standard 1, objective 3
Use the model periodic table provided to answer questions .
Use this
periodic
table to
answer
questions
1-11.
a1. What number of protons does the element “X” have?
A. 1
B. 4
C. 15
D. 19
If “X” has an atomic mass is 39, how many neutrons does it have?
a2.
A. 4
B. 8
C. 20
D. 22
3. How many electrons does “X” have?
A. 1
B. 4
C. 15
D. 19
c4. What similarities would you expect to see between “Z” and other elements in its group?
They would have similar:
A.
B.
C.
D.
atomic number
properties
names
atom mass
c5. What element on the table would you expect to be most chemically similar to “X”?
A. V
B. Y
C. X
D. W
a6. How are “X” and “V” alike?
A.
B.
C.
D.
their electrons have the same number of energy levels
they have the same number of electrons
they are the same size
they have isotopes with the same number of protons
d7. “X” and “W” are tested by placing a small piece of them in water. What would you expect to
see happen?
A.
B.
C.
D.
X and W will react the same in water
X will react more strongly than W
W will react more strongly than X
X will react and W will not.
c8. Chemists are looking for a non-reactive substance to fill a soft container to maintain its
shape. Which element would be the best substance?
A.
B.
C.
D.
X
V
U
Z
e9. Which substances would you group together as metals?
A.
B.
C.
D.
Y, Z, U
X, V, W
X, W
Y, V, X, W
e10. Which group of elements includes gases and does not conduct electricity or heat well?
A.
B.
C.
D.
metals
metalloids
nonmetals
radioactive elements
e11. Which element(s) would be classified as metalloids?
A.
B.
C.
D.
Z
Y
Z, Y
W, X
Use this information to answer the next three questions:
“Y” has an atomic number of 52. It has an isotope that has a mass of 127 and an
isotope with a mass of 128.
b12. What can you predict about its average atomic mass?
A.
B.
C.
D.
It is closer to 127 than 128
It is closer to 128 than 127
it is between 127 and 128
it is below 127
b13. How many protons and neutrons does the Y127 isotope have?
A.
B.
C.
D.
52 protons, 75 neutrons
75 protons, 52 neutrons
63 protons, 64 neutrons
63 neutrons, 64 protons
b14. If “Y” only has a small percentage of atoms that are Y127, what can you predict about its
average atomic mass?
A.
B.
C.
D.
It is closer to 127 than 128
It is closer to 128 than 127
it is between 127 and 128
it is below 127
Use a Periodic Table to answer the following questions.
a15. How many protons does the isotope Carbon-13 have?
A. 6
B. 11
C. 12
D. 13
a16. How many electrons orbit a Calcium atom?
A. 2
B. 20
C. 40.8
D. 6.02 x1023
a17. How many neutrons are in the nucleus of most Fluorine atoms?
A. 7
B. 9
C. 10
D. 19
b18. Deuterium and Tritium are isotopes of Hydrogen. What structural feature of these
isotopes makes them different?
A.
B.
C.
D.
The number of neutrons
The number of protons
The number of electrons
The type of bond they form
d19. Which statement about reactivity trends in groups of the periodic table is correct?
A.
B.
C.
D.
Reactivity is the same for each element in a group.
Reactivity increases and then decreases in each group.
Reactivity decreases going down each group.
Reactivity increases going down each group.
d20. Elements in the halogen group (group 7) all share what characteristic?
A.
B.
C.
D.
They all have similar reactivity
Their size is the same
They have three isotopes
They are all gasses