Fall 2013Chemistry: Final Exam Review Guide

Ms. Garcia

*************There will be 100 multiple choice questions on the final exam*****************

Atom + History

  • History (Chadwick, Thomson, Rutherford, Bohr)
  • Parts of atom (nucleus, electron, protons)

Density

  • Calculate density

Percent Error

  • Calculate percent error

Scientific Notation

  • Read and convert to scientific notation

Algebra and Conversions

  • Algebraic equations
  • Conversions: ex gallons to ounces, milliliters to liters
  • Qualitative vs. quantitative measurements

Electromagnetic Radiation

  • Define
  • Where does it come from
  • Colors of the visible spectrum
  • Different types of radiation

Matter

  • Techniques used to separate mixtures
  • Law of Conservation of Mass
  • Define element, compound, heterogeneous, homogenous, mixture, solution
  • Label: Reactants and Products in a chemical equation

Isotopes

  • Define
  • Calculate average atomic mass given isotop values

Periodic Table

  • Blocks (pdfs)
  • Trends(electronegativity, ionization energy, radius)
  • Period and group numbers
  • Finding and calculating atomic number, mass, protons, and electrons
  • Characteristics of groups (alkali metals, earth metals, transition metals, metalloids, halogens, noble gasses)
  • Metals vs. Nonmetals

Orbital Notation

  • Number of electrons in each orbital (spdf)
  • Finding orbital notation for elements

Bonding

  • Lewis dot structures (electron dot diagrams)
  • Is it an ionic or covalent bond?
  • Ionic (writing formulas, names)
  • Covalent (writing formulas, names)
  • Ions (which elements gain/lose electrons, how many do they gain/lose and why?)
  • VSEPR (tetrahedral, bent, planar)

Scientific Notation

Part A: Express each of the following in standard form.

5.2 x 103
9.65 x 10–4
6 x 101
1 x 10–1

Part B: Express each of the following in scientific notation.

8,000
0.00029
59
0.043

Part C: Compute the following. Express each of the following in scientific notation

(2.2 x 103) (8. 5 x 1014)
(8.1 x 1020) (9.5 x 10–5)
(8.4 x 102) (2.0 x 107)
(4.5 x 10-5) (6.0 x 105)
((8.6 x 10-1) + (4.5 x 102) x (-6.3 x 102))/(4.6 x 10-1)

Algebra

Solve for the given variable. Show ALL work in the space provided

1. a-b=6 b=_____ / 4. PQ = VW T=_____
T U
2. a-2b=c b=_____ / 5. a2+ b2= c2 b= _____
if A=3, c=5
3. 2(a-b)=3x +b b=_____ / 6. Simplify
miles x sec x hour
hour year sec

Metric Conversion

7. 25 Km = ____m

8. 2.5 m = ____cm

9. 1000L = _____ml

10. 0.51g = _____mg

11. 2.53 g = ____Kg

12. What is a qualitative measurement?

Examples:

13. What is a quantitative measurement?

Examples:

Percent Error

1. Experimental value = 1.24 g
Accepted value = 1.30 g / Answer:______
2. Experimental value = 1.24 g
Accepted value = 9.98 g / Answer:______
3. Experimental value = 252 mL
Accepted value = 225 mL / Answer:______
4. Experimental value = 22.2 L
Accepted value = 22.4 L / Answer:______
5. Experimental value = 125.2 mg
Accepted value = 124.8 mg / Answer:______

Density

  1. ______is the amount of matter an object has per specific area:
  2. Weight
  3. Mass
  4. Volume
  5. Density
  6. The density of water is 1g/cm3. A cube has a side of 5 cm. It has a mass of 250 grams. The density of the cube is
  7. 50g/cm3 and will float on water
  8. 2.0g/cm3 and will float in water
  9. 50g/cm3 and will sink in water
  10. 2.0g/cm3 and will sink in water
  11. A graduated cylinder contains 100 ml of a liquid. The mass of the graduated cylinder with the liquid is 145 grams. The mass of the graduated cylinder when empty is 45 grams. The density of the liquid is
  12. 0.69 g/ml
  13. 1.45g/ml
  14. 1g/ml
  15. Unable to calculate with this information
  16. Jose has 10 mL of silver while Alicia has 30 mL of silver. Which of the following is false?
  17. Alicia's sample has 3 times the density of Jose's sample
  18. Alicia's sample has 3 times the volume of Jose's sample
  19. Alicia's sample has 3 times the mass of Jose's sample.
  20. Jose's sample has 1/3 the mass of Alicia's sample
  1. The mass of an object is 5g. You find the displaced volume from the graduated cylinder to be 25ml. If the actual density of the object is 0.29, what is your percent error? Round to the nearest 10th.
  1. A cube has length of 7 cm a width of 8 cm and a height of 2 cm. It has a mass of 50g. What is its density? Round to the nearest 10th and include units
  1. The density of aluminum is 2.7 g/ml. If the aluminum has a volume of 20 ml, what is the mass of the aluminum? Round to the nearest 10th and include units
  1. Objects A and B have identical masses. Object A has a volume of 7.0 mL and object B has a volume of 8.5 mL. Which is more dense?
  1. A 60.0 mL sample of plastic has a density of 0.88 g/mL. Half of the sample is removed. What will the new density be? Round to the nearest 10th and include units
  1. Two pieces of candy occupy 2.1 ml of space. The red candy has a mass of 5g and the blue candy has a mass of 7g. Which piece of candy is more dense?
  1. The radius of Walter’s tennis ball is measured to be 6.90cm, and its mass is measured to be 175g. Determine its density.
  1. Calculate (3.5 x 103) (2.57 x 10-4). Round to the nearest 10th and be sure your response is in correct scientific notation.

Matter- Physical and Chemical Changes

  1. Which is the state of matter that has a definite shape and definite volume?

a. / solid / c. / gas
b. / liquid / d. / plasma
  1. Which is the state of matter that has an indefinite shape and definite volume?

a. / solid / c. / gas
b. / liquid / d. / plasma
  1. Which is the type of separation technique being demonstrated in the figure?

a. / crystallization / c. / filtration
b. / distillation / d. / chromatography
  1. Which is NOT a chemical change?

a. / a piece of wood is burned / c. / a bar of iron rusts
b. / an egg is cooked / d. / ingredients for a cake are stirred together
  1. All of the following are physical changes except:

a. / Cutting / c. / Burning
b. / Tearing / d. / Melting
  1. The basic building blocks of matter are:

a. / Protons / c. / Neutrons
b. / Electrons / d. / All of the above
  1. Which would you most likely observe in a chemical reaction:

a. / State of matter change (ex: liquid to solid). / c. / Change of shape
b. / No change in mass / d. / Gas given off
  1. Which of the following is classified as an element:

a. / Copper / c. / Water
b. / Rubber / d. / Table Salt
  1. Which is an example of a homogeneous mixture?

a. / salad / c. / vegetable soup
b. / Ice water / d. / fresh-squeezed orange juice (no pulp)
  1. Which is the separation technique that relies on the different boiling points of the parts of the mixture?

a. / filtration / c. / chromatography
b. / distillation / d. / crystallization
  1. A 25.0-gram sample of magnesium oxide contains 10.8 grams of magnesium. What is the percent of oxygen by mass in this compound?

a. / 89.2 % / c. / 43.2 %
b. / 14.2 % / d. / 56.8 %
  1. According to the Law of Conservation of Mass, in any chemical change

a. / the mass of reactants is greater than the mass of products
b. / the mass of reactants is less than the mass of products
c. / the mass of reactants is equal to the mass of products
d. / the masses of products and reactants have no predictable relationship
  1. Which is a chemical property of copper?

a. / has a boiling point of 2567° C
b. / reacts in air to form a green layer
c. / has the symbol Cu
d. / is a solid at room temperature
  1. Which of the following substances is an element?

a. / Baking soda / c. / Salt
b. / Iron / d. / Sugar
  1. Which of the following formations is a physical property of copper?

a. / A deep blue solution when in contact with ammonia.
b. / A new substance when combined with nitric acid.
c. / A green copper carbonate compound when in contact with moist air.
d. / A formation of a drill gauge and wire.
  1. Which of the following can be classified as a heterogeneous mixture?

a. / Trail Mix / c. / Alcohol
b. / Faucet Water / d. / Coffee
  1. In the physical and chemical changes lab, you added a piece of magnesium to hydrochloric acid. The following depicts the reaction: 2HCl + Mg → MgCl2 + H2. Is this characterized as a chemical or physical reaction?

a. / Chemical / b. / Physical
  1. When wax from a candle melts the state of matter changes from a solid to a liquid. Is this a chemical or physical reaction?

a. / Chemical / b. / Physical
  1. When do we use evaporation to separate components?

a. / A solid-liquid mixture when solid particles are dissolved / c. / A liquid-solid mixture when solid particles can be seen in the mixture.
b. / A solid-solid mixture when one of the components sublimes (solid straight to gas…like dry ice) / d. / A liquid-liquid mixture when one of the liquids has a lower boiling point.
  1. If I know the components of a mixture and the boiling points of the components, which is a possible way to isolate the components in the mixture

a. / Make use of evaporation / c. / Make use of paper chromatography
b. / Make use of magnetic attraction / d. / Make use of distillation

Atoms and Subatomic Particles

Write the symbol for an atom or ion with the following subatomic particles. Include the mass number, atomic number, and charge, if any.

11. 28 protons, 26 electrons, 30 neutrons

  1. Mass number 89, 36 electrons, 51 neutrons
  1. 20 protons, 18 electrons, 20 neutrons
  1. 14 neutrons, 13 protons, 13 electrons
  1. Mass number 132, 78 neutrons, 54 electrons
  1. The atomic mass of fluorine is 18.9984 amu and that of copper is 63.546 amu. All fluorine atoms have a mass of 18.9984 and not a single copper atom has a mass of 63.546 amu. Explain.
  1. The natural abundance for boron isotopes is: 19.9% 10B (10.013 amu) and 80.1% 11B (11.009amu). Calculate the atomic weight of boron. Show ALL your work!
  1. Calculate the weight of silicon using the following data for the percent natural abundance and mass of each isotope: 92.23% 28Si (27.9769 amu); 4.67% 29 Si (28.9765); 3.10% 30Si (29.9738 amu). Show ALL your work!

19. You calculated the atomic mass of potassium (K) to be 41.23 amu. Using the actual value from the periodic table, what is your percent error?

  1. The identity of an element can be determined on the basis of which of the following?
  1. the number of neutrons in an atom of the element
  2. the number of protons in an atom of the element
  3. the mass number of the element
  4. the atomic mass of the element
  1. Which of the following was originally Dalton’s atomic theory, but had to be revised about a century ago?
  1. Atoms are tiny indivisible particles.
  2. The atoms of one element are different from those of any other element.
  3. Compounds are made by combining atoms.
  4. Atoms of different elements can combine with one another in simple whole number ratios.
  1. Rutherford proposed a model of the atom with a very small, dense nucleus after conducting which experiment?
  1. Plum pudding experiment
  2. Photoelectric effect
  3. Gold foil experiment
  4. Schrödinger’s cat
  1. All atoms of the same element have the same ______.
  1. number of neutrons
  2. number of protons
  3. mass numbers
  4. mass
  1. The atomic mass of an element is the ______.
  1. total number of subatomic particles in the nucleus
  2. weighted average of the masses of the isotopes of the element
  3. total mass of the isotopes of the element
  4. average of the mass number and the atomic number for the element
  1. All atoms with 20 protons are
  1. electrically neutral
  2. positively charged
  3. neon
  4. calcium
  1. The piece of information that IS NOT on the periodic table is
  1. Element symbol
  2. Mass number
  3. Atomic number
  4. Atomic mass
  1. The scientist credited with developing the “solar system” model of the atom where electrons circle the nucleus in orbits is:
  1. Aristotle
  2. Milliken
  3. Bohr
  4. Schrödinger
  1. The first scientist to show that atoms emit tiny negative particles was
  1. J.J. Thomson
  2. Robert Boyle
  3. Ernest Rutherford
  4. John Dalton
  1. The scientist whose alpha-particle/gold foil experiment led him to conclude that the nucleus of an atom contains a dense center of positive charge is

A.J.J. Thomson

B.Robert Boyle

C.Ernest Rutherford

D.John Dalton

  1. The number 80 in the name bromine-80 represents
  1. the atomic number
  2. the mass number
  3. the year of the element’s discover
  4. none of the above
  1. The particles that are found in the nucleus of an atom are ______.
  2. protons only
  3. electrons only
  4. protons and neutrons
  5. protons, neutrons, and electrons

32. The mass number of an atom equals

  1. the number of neutrons per atom
  2. the atomic mass of the element
  3. the atomic number of the element
  4. the number of protons plus the number of neutrons per atom

33. J.J Thompson first described a positively charged filled atom with negatively mixed charges spread throughout. He called this the:

A. Atomic Theory

B. String Theory

C. Nucleus

D. Plum-Pudding Model

A. Atomic Mass / B. Nucleus / C. Atom / D. Neutron
E. Atomic Number / F. Proton / G. Electron / H. Isotope
I. Mass #
34. / The smallest particle of an element that retains the properties of that element
35. / A positively charged subatomic particle
36. / A negatively charged subatomic particle
37. / A subatomic particle with no charge
38. / The central part of an atom, containing protons and neutrons
39. / Atoms with the same # of protons, but different # of neutrons in the nucleus of an atom
40. / The total number of protons and neutrons in the nucleus of an atom
41. / The number of protons in the nucleus of an element
42. / The weighted average of the masses of the isotopes of an element

Define isotope: ______

Symbol / Atomic Number / Number of Protons / Number of Neutrons / Number of Electrons / Mass #
1 /

60Cu+2

2 /

30Si

3 /

19F-

4 / 18 / 22 / 18
5 /

67Cu+2

6 /

82Br-1

7 /

99Mo+

8 / 34 / 36 / 44
9 / 78 / 54 / 75 / 132
10 / 20 / 20 / 18

Periodic Table + Trends

True or False

  1. Elements in the same period tend to have the same number of valence electrons.
  2. Elements in Group 17 are classified as halogens.
  3. Elements in Group 2 are classified as alkali metals.
  4. Group I consists of non-metals
  5. Group IV consists of metals, nonmetals, and metalloids.
  6. Nitrogen is a metal
  7. Potassium is a metal
  8. Antimony and silicon are metalloids
  9. Aluminum is a metalloid
  10. Cobalt is considered a transition metal
  11. Calcium resides in period 3
  12. In general, metals prefer to receive electrons
  13. Francium is probably not a good conductor of electricity
  14. Carbon is malleable
  15. Carbon and silicon can gain or lose electrons during bonding.
  16. Neon resides in period 2

Multiple Choice

  1. Which region is referred to as the p-block on the diagram?

a. / A / c. / C
b. / B / d. / D
  1. Which region is referred to as the f-block on the diagram?

a. / A / c. / C
b. / B / d. / D
  1. Which region contains the halogen family of elements?

a. / A / c. / C
b. / B / d. / D
  1. Which region contains the alkaline earth metal family of elements?

a. / A / c. / C
b. / B / d. / D
  1. Which region contains elements with two valence electrons?

a. / A / c. / C
b. / B / d. / D
  1. Which region contains elements with an electron configuration

ending in p3?

a. / A / c. / C
b. / B / d. / D
  1. Which block on the periodic table contains the actinide series of

elements?

a. / s-block / c. / d-block
b. / p-block / d. / f-block
  1. Which diagram correctly depicts the

trend in electronegativity?

a. / a / c. / c
b. / b / d. / d
  1. Which diagram correctly depicts the

general trend in ionization energy?

a. / a / c. / c
b. / b / d. / d
  1. Which diagram correctly depicts the

general trend in atomic radius?

a. / a / c. / c
b. / b / d. / d
  1. Which element has valence electrons residing

in the third energy level?

a. / A / c. / C
b. / B / d. / D
  1. Identify the period and group numbers of the element with the electron configuration. [Ne]3s23p4

a. / Period 2, Group 4 / c. / Period 3, Group 16
b. / Period 3, Group 4 / d. / Period 2, Group 16
  1. Which correctly describes elements in the same group?

a. / They have the same number of valence electrons.
b. / They have electrons in the same outermost energy level.
c. / They have the same atomic radius.
d. / They must be in the same state of matter.
  1. Which is the halogen that is in Period 5?

a. / Bromine (Br) / c. / Iodine (I)
b. / Strontium (Sr) / d. / Xenon (Xe)
  1. Which metalloid is in the fourth period and the same group as Carbon?

a. / Silicon / c. / Tin
b. / Germanium / d. / Boron
  1. Which is the most important characteristic in determining an element’s chemical properties?

a. / the number of protons and neutrons in its nucleus
b. / which period it is found in
c. / the number of valence electrons it contains
d. / its outermost energy level
  1. Which property describes how much energy must be added to an atom to remove an outermost electron?

a. / atomic radius / c. / electronegativity
b. / ionic radius / d. / ionization energy
  1. How many valence electrons does Pb (lead) have?

a. / 1 / c. / 3
b. / 2 / d. / 4
  1. How many valence electrons does an element in Group VII have?

a. / 4 / c. / 6
b. / 5 / d. / 7
  1. How many valence electrons do the noble gasses have?

a. / 5 / c. / 7
b. / 6 / d. / 8
  1. How many valence electrons does an element whose outer shell configuration is 3p3 have?

a. / 5 / c. / 7
b. / 6 / d. / 3
  1. How many valence electrons does an element whose outer shell configuration is 4p6 have?

a. / 5 / c. / 7
b. / 6 / d. / 8
  1. An extremely reactive element would probably have what type of outer shell configuration?

a. / 2s1 / c. / 2p1
b. / 3s3 / d. / 4p6
  1. The energy needed for an electron to be pulled from an atom is called:

a. / Electronegativity / c. / Ionization Energy
b. / Polarity / d. / Magnetic Energy
  1. Which element below is the MOST electronegative?

a. / C / c. / O
b. / N / d. / F
  1. Which element below is the MOST electronegative?

a. / C / c. / Ge
b. / Si / d. / Sn
  1. Which element below has the LARGEST radius?

a. / C / c. / O
b. / N / d. / F
  1. Which element below has the LARGEST radius?

a. / C / c. / Ge
b. / Si / d. / Sn
  1. Which element below has the HIGHEST ionization energy?

a. / C / c. / O
b. / N / d. / F
  1. Which element below has the HIGHEST ionization energy?

a. / C / c. / Ge
b. / Si / d. / Sn
  1. Group I is also know as the

a. / Alkali Metals / c. / Alkaline Earth Metals
b. / Noble gasses / d. / Halogens
  1. Group VII is also know as

a. / Alkali Metals / c. / Alkaline Earth Metals
b. / Noble gasses / d. / Halogens
  1. Chlorine is a(n)

a. / Alkali Metal / c. / Alkaline Earth Metal
b. / Noble gass / d. / Halogen
  1. Which group listed below contains the MOST reactive elements:

a. / Group I / c. / Group III
b. / Group IV / d. / Group VIII
  1. Which group listed below contains the LEAST reactive elements:

a. / Group I / c. / Group III
b. / Group IV / d. / Group VIII
  1. What element has the following electron configuration 4p3:

a. / Se / c. / N
b. / Sb / d. / As
  1. What element has the following electron configuration 3s3:

a. / Mg / c. / Na
b. / Al / d. / No such element

  1. What family is represented by the letter “A” elements:

a. / Halogen / c. / Lanthanides
b. / Actinides / d. / Nonmetals
  1. What family is represented by the letter “B” elements:

a. / Halogen / c. / Lanthanides
b. / Actinides / d. / Nonmetals
  1. Elements in Group III will want to:

a. / Gain 3 electrons / c. / Lose 3 electrons
b. / Gain 5 electrons / d. / Lose 5 electrons
  1. Elements in Group VI will want to:

a. / Gain 2 electrons / c. / Lose 2 electrons
b. / Gain 6 electrons / d. / Lose 6 electrons

Electron Notation

  1. Which is the correct electron configuration notation for Nitrogen (N)?
  1. Which is the correct electron configuration notation for Chlorine (Cl)?
  1. Which is the correct electron configuration notation for Bromine (Br)?
  1. What do the numbers 1-7 stand for in an electron configuration?
  2. Electrons
  3. Protons and Neutrons
  4. Energy Levels
  5. Orbitals
  1. What do the letters s,p,d and f stand for in an electron configuration?
  2. Electrons
  3. Protons and Neutrons
  4. Energy Levels
  5. Orbitals
  1. What are the colors of the visible light spectrum in order starting with RED!
  1. List three different types of electromagnetic waves we learned about?
  1. Explains how electrons produce electromagnetic waves
  1. Why does every element on the periodic table have a unique electromagnetic spectra?
  1. Which of the following correctly represents the orbital notation in the “d” orbital for Cobalt (Co)?
  1. The “up” and “ down” arrows in an electron orbital notation depict:
  2. Protons and neutrons in orbitals
  3. Electrons with opposite spins
  4. Oppositely charged electrons
  5. Electrons and protons attracting each other
  1. Give the electron configuration notation for: Ca2+
  1. Give the electron configuration notation for Cl -1
  1. Draw the orbital notation for Magnesium (Mg)
  1. Draw the orbital notation for Sulfur (S2-)
  1. How many electrons can the d orbital hold?
  1. How many electrons can the 3s orbital hold?
  1. Explain why atomic orbital 5s comes before 4d?
  1. A “stable” electron configuration is likely to contain:
  2. Filled energy sublevels
  3. Fewer electrons than unstable configurations
  4. Unfilled s orbitals
  5. Electrons with clockwise spin
  1. How many unpaired electrons are in a rubidium (Rb) atom?
  1. How many unpaired electrons are in a krypton (Kr) atom?

Covalent, Ionic, and Metallic Bonding