Final Exam Review Name: ______________________ History, the Scientific Method and Measurements: Measurements: 16) How much fluid is in the graduated cylinder to the right? Please note: the graduated cylinder measures in milliliters. ___________________ 17) How much fluid is in the graduated cylinder to the left? Please note: the graduated cylinder measures in milliliters. ______________________ 18) How much mass must be on the metal platform if the triple-­‐beam balance below is balanced? Mass = _________________ 19) How much mass must be on the metal platform if the triple-­‐beam balance to the right is balanced? Mass = _________________ Please answer the following question based on the graph below (1pt each unless specified otherwise): 20) What does this graph show? 21) What is the independent variable? 22) What is the dependent variable? 23) Is it ok to connect the data points in this graph? Why or why not? (2 pts) 24) What is the temperature of the water at 10 minutes? 25) Lorraine calculated that the mean temperature of the pot was 10 degrees Celsius. Is she right? Why or why not? (2pts) 26) Are the following research questions testable? If so, what is the dependent variable? If not, please re-­‐write them as a testable research question. (3 pts each) Does the amount of water affect how fast sugar will dissolve in water? (y) (n) Do tomatoes that are given more water taste better than those that are given less water? (y) (n) 27) Given the following research question, please identify the Independent Variable, the Dependent Variable, and write a possible hypothesis. (3 pts) Does the height a basketball’s bounce depend on the air pressure in the ball? Dependent Variable: ____________________________________________________ Independent Variable: __________________________________________________ Hypothesis: 28) Jeremiah wanted to see if skittles dissolve faster than M&M’s do. He realized he made a mistake last time and fixed one of his problems. This time, he bought a bag of skittles and a bag of M&M’s. He carefully measured out 1 cup of warm water and 1 cup of cold water. He put 5 green M&M’s in the cold water, and at the same time, put 7 green skittles in the warm water. He then used a stop watch to determine which candy dissolved fastest. What did he do wrong this time? How should he correct his experiment? 29) Read each observation below. Circle whether the observation is qualitative or quantitative. If it is qualitative, rewrite it as a quantitative observation. If it is already quantitative, write down what you would measure. (2 pts each) Lisa lost seven pencils last week (quant.) (qual.) Most of a chimp’s diet comes from fruit (quant.) (qual.) After the chemical was added, the water became warm (quant.) (qual.) 30) Read each observation below. Then write an inference that could explain the observation. (1 pt each) The teacher hands Alysha her test back and Alysha smiles You call a friend, and your friend does not pick up the phone 31) Examine the data set shown below. Then give a brief summary of what the experimenter can conclude from the data: (2pts) Distance from # baskets the hoop (meters) made 1 12 2 10 3 9 4 5 32) Why is saying that “the reason the number of baskets decreases is because the shots are more difficult” not a conclusion supported by the table above? (2pts) CONSERVATION LAWS AND ELEMENTS Please select the chemical symbol for the following elements: 1) Aluminum: a) Al b) Au c) Ag d) A 2) Chlorine: a) C b) Cl c) Ch d) Na 3) Calcium: a) C b) Cl c) Ca d) Cu 4) Carbon: a) C b) Cl c) Ca d) Cu 5) Copper: a) C b) Co c) Ca d) Cu 6) Gold a) G b) Au c) Ag d) Go 7) Helium a) He b) H c) Hl d) Hi 8) Hydrogen a) He b) H c) Hy d) Pb 9) Iron a) Ir b) I c) Fe d) Au 10) Lead a) L b) Le c) Pb d) Hg 11) Mercury a) M b) Me c) Pb d) Hg 12) Nitrogen a) N b) Ni c) Au d) Ag 13) Oxygen a) O b) Ox c) Oy d) Fe 14) Potassium a) P b) Pu c) K d) U 15) Sulfur a) S b) Su c) Na d) So 16) Sodium a) S b) So c) Na d) Su 17) Uranium a) U b) Ur c) Hg d) Fe 18) Plutonium a) P b) Pl c) Pu d) U True or False: Please select the best answer. If it is false, CHANGE IT TO MAKE IT TRUE 19) (T) (F) In a closed system during a chemical change, mass is always conserved. 20) (T) (F) In a closed system during a chemical change, volume is always conserved. 21) (T) (F) In an open system during a chemical change, the measured mass is always the same before and after the reaction. 22) (T) (F) In a closed system when a solid melts, mass is always conserved. 23) (T) (F) In an open system when a solid melts, mass is always conserved. 24) (T) (F) In an open system during any physical change, the measured mass is always the same before and after the reaction. 25) (T) (F) In a closed system when a solid dissolves, volume is always conserved. 26) (T) (F) In a closed system when a solid dissolves, mass is always conserved. 27) (T) (F) If you melt ice in a closed zip-­‐lock bag, both the mass and volume of the water molecules will stay the same. 28) (T) (F) If you dissolve sugar in hot cup of tea, that is a closed system. 29) (T) (F) In a nuclear reaction in a closed system, mass is always conserved 30) (T) (F) If you burn a candle in a closed system, such as a sealed, large jar, the mass will decrease as the candle burns. 31) (T) (F) If you boil water in a pot on the stove, the mass of water in the pot will stay the same over time. 32) (T) (F) If you melt M&M’s in a sealed ziplock bag in the microwave, the mass has to stay the same. 33) (T) (F) 34) (T) (F) 35) (T) (F) 36) (T) (F) 37) (T) (F) 38) (T) (F) 39) (T) (F) 40) (T) (F) 41) (T) (F) 42) (T) (F) 43) (T) (F) 44) (T) (F) 45) (T) (F) If you melt M&M’s in a sealed zip-­‐lock bag in the microwave, the volume has to stay the same. When the U.S. dropped Fat Man, a nuclear bomb, on Nagasaki in World War II, all the mass of the bomb after the explosion was the same as all of the mass of the bomb before the explosion. When you burn wood in a campfire, the mass of the ashes equals the mass of the wood before it burned. When you burn wood in a campfire, the mass decreases because some of the atoms are destroyed. When you burn wood in a campfire, the mass decreases because the gasses that are created are free to move away. If you dissolve baking soda with an acid, such as vinegar, the gas that is created is CO2, or carbon dioxide. The sun is constantly losing mass because it is burning hydrogen and oxygen in an open container. The sun is constantly losing mass because it is converting mass into pure energy. The reason that you can smell a Thanksgiving turkey cooking in the oven is because the oven is an open system. The mass of the water lost in a puddle to evaporation is the same as the mass gained by the atmosphere. The mass of water lost by the ocean to evaporation is more than the mass gained by the atmosphere. The volume taken up by cooled lava has to be the same as the volume taken up by molten lava. The mass of lava cooling on the beach has to be the same as the mass of the magma under the ground before the eruption. Properties of Pure Substances: Multiple Choice / fill in the blank: 1 point per part. Please circle the correct answer. 27) A material that has melted has gone through a (chemical) (physical) change. 28) A material that has been burned has gone through a (chemical) (physical) change. 29) A (heterogeneous) (homogeneous) mixture is a mixture where you can see and easily separate the individual parts. 30) A (heterogeneous) (homogeneous) mixture is a mixture where the parts are so evenly mixed that you can’t see the individual parts. 31) A (physical) (chemical) property is a characteristic of a substance that can be observed without changing it into any other substance. 32) A (physical) (chemical) property is a property of a substance that describes its ability to change into different substances. 33) Glass is an example of a(n) (amorphous) (crystalline) solid 34) Salt is an example of a(n) (amorphous) (crystalline) solid. 35) (1 pt) The pressure is greater at the bottom of (a small, deep pond) or a (huge, shallow lake). 36) (true) (false) A submerged object displaces more volume of liquid than its own volume. 37) Archimedes principle says that an immersed object is pushed (up) (down) by a force equal to the (weight) (volume) (mass) of the fluid it displaces. 38) A salad is an example of a (homogeneous) (heterogeneous) mixture. 39) Below is the phase diagram for Carbon Dioxide: a) At point E (under very high pressure), if you decrease the temperature, the CO2 first turns into a ________________ and then eventually turn into a _________________ b) At point D, if you increase the pressure, it first goes from a _____________ to a ______________ through the process of ____________________ c) At point A, if you increase the temperature, you go from a ____________ to a ______________ through the process of ___________________ d) What is the lowest temperature that liquid CO2 can exist at? ______________ 40) Please answer the questions below using the water cycle figure to the right. A) The process that turns water vapor into clouds: ___________________ B) The process of liquid water flowing on the surface back to the ocean: ____________________ C) The process of water falling back to the surface of the earth: _____________________ D) The process of water going from “on the surface” to “in the ground”: _______________ E) Water that is stored in the ground: ______________________ Math Problems (2 pts each): You must show your work to receive full credit. Writing down a number will only give you half-­credit! You must include the correct unit! ρ = m / v 41) What is the density of a rock that has a volume of 3ml and a mass of 15 grams? 42) What is the mass of a piece of gold that has a volume of 3cm3 and a density of 19.3 g/cm3? 43) What is the volume of a necklace that has a density of 7 g/cm3 and a mass of 35g? 44) Please use the change of state graph below to answer the following questions: a) On the change of state graph, below, please label where the material is a: solid liquid gas boiling melting freezing condensing b) Assuming the material is water, what are the temperatures of the two plateaus here in Los Alamos? (Deg. C) upper: ____________ lower: _____________
Long Answer: Answer 3 of the 5 questions. You must answer in complete sentences, and you must restate the question in your answer. 3 points each. BE AS SPECIFIC AS WE WERE IN CLASS! You may answer one additional question for extra credit. 45) Based on the Kinetic Molecular Theory, why does the fluid level in a thermometer rise when it is heated? 46) Based on the Kinetic Molecular Theory, why does a crystalline solid turn into liquid at a specific temperature? Why does an amorphous solid not melt at a specific temperature? 47) Based on the Kinetic Molecular Theory, why are most solids more dense than their liquid form? What is an extremely important exception to this rule? 48) Why do bridges have “thermal expansion joints”? 49) A student takes some salt water and fresh water, as shown in the picture to the right. The cork floats on top of the fresh water, and the fresh water on top of the salt water. The egg floats between the salt water and fresh water, and a quarter sinks all the way to the bottom. a) Please arrange the items from most dense to least dense (just arrange, not complete sentences). b) Scientifically, how do you know that this is the case? (complete sentences) History and Structure of the Periodic Table Name: ___________________ Period: __________________ The Periodic Table and Elements Unit Test 1) The small region at the center of the atom where the positive charge is concentrated is
called the ______.
a) proton
b) neutron
c) electron
d) nucleus
e) atom
2) The positively charged particles that are in an atom’s nucleus are called _______.
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
3) The answer is “a”
4) The small, negatively charged particles in an atom are called _______.
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
5) _______ are the smallest particles that can still be considered an element.
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
6) Thomson proved that atoms must have small, charged particles called:
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
7) Rutherford’s gold foil experiment proved that the _______ are concentrated in the
nucleus of an atom.
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
8) Bohr’s experiments lead him to conclude that the _________________ are not free to
move wherever they want, but are constrained to specific orbits.
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
9) The ______________ have no charge, and are found in the nucleus of an atom.
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
10) There must be the same number of protons and ________________ in an atom for it
to be electrically neutral.
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
11) The number of ______ in an element is known as the atomic number of the element.
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
12) The atomic mass of an atom is the sum of the number of protons and ______ in that
atom.
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
13) All atoms of a specific element must have the same number of _______ but can have
slightly varying numbers of neutrons.
a) protons
b) neutrons
c) electrons
d) nucleus
e) atoms
14) Atoms with the same number of protons but a different number of ______ are called
isotopes of that element.
a) protons
b) neutrons
c) electrons
15) Lithium-7 has ___ protons.
a) 3
b) 4
c) 7
d) 14 e) 1
16) Lithium-7 has ___ neutrons.
a) 3
b) 4
c) 7
d) 14 e) 1
17) Lithium-7 has ___ electrons.
a) 3
b) 4
c) 7
d) 14 e) 1
d) nucleus
e) atoms
18) Lithium-7 has ___ electrons in its outermost shell.
a) 3 b) 4 c) 7 d) 14 e) 1
19) Lithium-7 has an atomic number of ___.
a) 3
b) 4
c) 7
d) 14 e) 1
20) Lithium-7 has an atomic mass of ___
a) 3
b) 4
c) 7
d) 14 e) 1
21) The most reactive metals are known as the _____ metals.
a) Halogens b) Alkaline Earth
c) Transition d) Lanthanides e) Alkali
22) Elements that are grouped vertically in columns are in the same ____________. a) group b) period c) township d) street e) row 23) Elements that are grouped horizontally in rows are in the same _____________. a) group b) period c) township d) street e) row 24) Elements that have the same number of electron shells are in the same ______. a) group b) period c) township d) street e) row 25) Elements that have an atomic number greater than 92 are known as the ___________ elements. a) Alkali b) Transition c) Transuranium d) Lanthanide 26) The shininess and reflectivity of a metal is known as its ____. a) dactility b) ductility c) luster d) malleability 27) A material that is able to be hammered or rolled into flat shapes is ________________. a) dactile b) ductile c) luster d) malleable 28) A material that can be stretched into thin wires is _______________________. a) dactile b) ductile c) luster d) malleable 29) The force that is pushing the nucleus apart is the _____ force.
a) strong nuclear
b) electric
c) magnetic d) protonic
30) The force that holds the nucleus together is the _____ force.
a) strong nuclear
b) electric
c) magnetic
d) protonic
31) ______ particles are large, positively charged radioactive particles that consist of two
protons and two neutrons.
a) alpha
b) beta
c) gamma
d) x-rays
e) light
32) ____ particles are electrons being shot out from the nucleus.
a) alpha
b) beta
c) gamma
d) x
e) light
33) ______ rays are high-frequency “light” emitted from the nucleus.
a) alpha
b) beta
c) gamma
d) x-rays
e) light
34) A nuclear reaction where the nuclei split apart: ________.
a) fission
b) fusion
c) nuclear
d) Fermi
e) sun
35) A nuclear reaction where nuclei combine to make a bigger nuclei: _________.
a) fission
b) fusion
c) nuclear
d) Fermi
e) sun
36) The sun gets its power from a ____ reaction.
a) fission
b) fusion
c) nitrogen
d) Fermi
e) gamma
37) The atomic bombs that were dropped on Japan were ___ bombs.
a) fission
b) fusion
c) hydrogen
d) Fermi
e) gamma
True / False. Remember, a statement is false if any part of the statement is untrue. 38) ___ The nucleus of an atom contains both protons and electrons.
39) ___ If carbon has 6 protons and 6 neutrons its atomic mass is 12 and its atomic
number is 6.
40) ___ Protons and neutrons have almost the same mass.
41) ___ Protons and electrons have almost the same mass
42) ___ Almost all the mass of an atom is concentrated in the electron cloud, because it is
so big.
43) ___ Almost all the volume of an atom is concentrated in the electron cloud, because it
is so big.
44) ___ Oxygen-­‐16 has 8 protons, 8 neutrons, 8 electrons, an atomic mass of 8 and an atomic number of 16. 45) ___ Gold is highly conductive, shiny and brittle. 46) ___ Because copper, gold and silver are all in the same group, they should have similar properties. 47) ___ Alkali metals are the most reactive elements. 48) ___ Because lithium reacts violently with water, we say it has a low reactivity, because it takes a short period of time to react. 49) _____ The strong nuclear force only operates on very small scales. 50) _____ There are four types of radiation emitted from the nucleus: alpha particles, beta particles, gamma rays and x-­‐rays. 51) ______ If a radioactive element has a half-­‐life of 22 days, then, in a given sample, all of the material will be gone in 22 days. 52) _____ If a radioactive element has a half-­‐life of 22 days, then, in a given sample, 3/4 of the material will be gone in 44 days. 53) _____ The two main forces in the nucleus are the strong nuclear force and the magnetic force. 54) _____ Different elements have different half-­‐lives because they have different numbers of protons and neutrons. 55) _____ Different isotopes of the same element have the same half-­‐life, because they have the same number of protons. 56) _____ Fusion is the primary form of nuclear reactions that stars use to get energy. 57) _____ Uranium and plutonium bombs operate on the principal of fission. 58-­‐67) Oxygen has _____ electron shell(s) and _____ electron(s) in its outermost shell. It needs ____ electron(s) to completely fill its outermost shell, so it will bond with ____ sodium molecule(s) or _____ calcium molecule(s). Oxygen has an isotope, Oxygen-­‐15, which has _____ protons, _____ neutrons, and ____ electrons. This isotope, Oxygen-­‐15, has an atomic number of _____ and an atomic mass of ______. 68) Please draw me a picture of Beryllium-­‐7, using for protons, for electrons and for neutrons. Be sure to put the correct number of electrons in each orbital / shell / energy level. 69-­‐77) Alkali Metals: ______ Alkali Earth Metals: _____ Mixed Group Metals:_____ Lanthanides: ______ Actinides: _______ Metalloids: _______ Transition Metals: ______ Halogens: ______ Noble Gasses: _____ ANSWER BELOW ON A SEPARATE SHEET OF PAPER 78) Why are large nuclei more unstable and likely to break apart (undergo fission) than smaller nuclei are? Be specific. Tell me about the forces involved, the distances they operate over, what the forces do, and how that all comes together to make an atom unstable. 79) Why, as you go vertically down the periodic table, do the atoms get larger? How and why does this affect their reactivity (NOT radioactivity)? Why, as you go horizontally (from left to right) across the periodic table, do the atoms get smaller, even though you are adding more electrons and protons to the atom? 80) In your high-­‐school chemistry class, you perform a series of chemical reactions to isolate an element. When you filter out the element, it forms little flakes that are shiny and malleable. However, the flakes have a low melting point and react violently with water. They also float on top of the water. What type of an element is this? And would you expect it to conduct electricity? Be sure to explain why for all your responses. Elements, Compounds, Mixtures, Solutions 16) (1pt) Chlorine and sulfur react together to form an (ionic) (covalent) bond. 17) (2 pts) Please draw the electron dot diagram for chlorine and sulfur, one of each atom, individually: 18) How many sulfur atoms and chlorine atoms will you need for the bond listed above? # of sulfur: _______ # chlorine: ________ 19) (3 pts) Use an electron dot diagram to show how the chlorine atom(s) and sulfur atom(s) will bond: 20) Which elements are more reactive, those in chlorine’s group, or those in sulfur’s group? (Sulfur’s) (Chlorine’s) 21) Which group’s atoms want electron’s more? (Sulfur’s) (Chlorine’s) 22) Which atom is more electronegative? (Sulfur) (Chlorine) Lithium / Oxygen 23) Lithium and oxygen will react to form a compound. Will it be (ionic) or (covalent)? 24) (2 pts) Draw the electron dot diagrams for an atom of lithium and an atom of oxygen: 25) (2 pts) When they react, which atom will become positive? Why? 26) (2 pts) Draw the electron dot diagram showing this: 27) (2 pts) You will need _______ oxygen atoms and ______ lithium atoms to make sure that the total charge is zero. 28) What is the chemical formula for this compound? _________________ 29) What is the chemical name for this compound? _____________________________________ Oxygen -­ Oxygen 30) Draw the electron dot diagram for when two oxygen atoms come together to form an oxygen molecule. 31) The bond between the two oxygen atoms is a (single) (double) (triple) bond. 32) (2 pts) Why is the bond between the two oxygen atoms non-­‐polar? 33) Is this an ionic or covalent bond? Why? 34) Why do covalently-­‐bonded molecules tend to have low boiling and melting points, while ionic compounds have high melting points? Why do non-­‐polar, covalently-­‐bonded molecules, such as nitrogen or oxygen, have extremely low melting and boiling points? Please be sure to include a diagram with charges or partial charges located on the atoms. ENERGY: 6) How much potential energy does a 2kg object have if it is 2m above the ground? (PE = m*g*h g = 9.8 m/s2) 7) How much kinetic energy does a 2kg object have if it is has a speed of 4m/s? (KE = ½ m*v2) 8) (3 pts) What is the velocity of an object, if it falls 5 meters? Assume that gravity is 10 m/s2 , not 9.8 m/s2. You must show your work to get full credit. Short Answer: You must answer in complete sentences. You may also use a drawing if you feel it will help (2 pts each). You must also restate the question in your answer. 6) Why is thermal energy considered to be a form of kinetic energy? 7) Why is chemical energy considered to be a type of potential energy? Where is the energy stored? Math-­y questions (2 pts each): 8) Lightbulb A gets 100 joules of energy. It converts 80 joules of the energy into light energy. Lightbulb B also gets 100 joules of energy. It converts 60 joules of the energy into light. Which lightbulb is more efficient? Why? 9) Lightbulb A gets 100 joules of energy. It converts 80 joules of energy into light. Lightbulb B gets 200 joules of energy. It converts 180 joules of energy into light. Which lightbulb is more efficient? Why? 10) Lightbulb A converts electric energy only into electromagnetic energy and thermal energy. It gets 100 joules of electric energy and turns it into 80 joules of light. How much energy had to be converted into thermal energy? Why? Energy conversions: Please tell me the main type of energy each object uses, and what the main type of energy the object converts the energy into. (2 pts each) 11) Uses: ___________________________ SPEAKER Changes into: _________________ 12) Uses: ___________________________ CAR Changes into: _________________ ALSO KNOW INFO ON 2 MOST RECENT QUIZZES (ELECTRICITY, MAGNETISM, WAVES, SOUND, LIGHT)