Download Name: (1 of 2) Math Set # 13 Protons, Neutrons, Electrons Proton

Name: ____________________________________
(1 of 2)
Math Set # 13 Protons, Neutrons, Electrons
Proton = positive particle in the nucleus of an atom
Neutron = positive particle in the nucleus of an atom
Electron = negative particle moving around the outer edge of an atom
Atomic Number = the number of protons
Atomic Mass = the number of protons plus the number of neutrons
EXCEPT FOR IONS the number of protons = the number of electrons
1. An atom with an atomic number of 8 has 8 of what particle?
2. An atom with an atomic number of 76 has 108 of what particle?
3. An atom with an atomic mass of 20 has 20 of what particles?
4. An atom with an atomic mass of 11 has 11 of what particles?
5. An atom is NOT an ion. It contains 12 protons. How many electrons does it have?
6. An atom is NOT an ion. It contains 58 protons. How many electrons does it have?
7. An atom is NOT an ion. It has an atomic number of 33. How many electrons does
it have?
8. An atom is NOT an ion. It has an atomic number of 1. How many electrons does
it have?
Name: ____________________________________
(2 of 2)
Math Set # 13 Protons, neutrons, electrons
# protons = atomic number (ALWAYS)
# electrons = # protons (EXCEPT FOR IONS)
# neutrons/protons = atomic mass
# neutrons = atomic mass minus atomic number
Example:
An atom of Oxygen has an atomic number of 8 and an atomic mass of 16. It is not an
ion. Give the number of protons, neutrons, and electrons
ANSWER:
Protons = 8 (atomic number)
Electrons = 8 (number of protons)
Neutrons = 16 proton/neutrons – 8 protons = 8 neutrons
1. Give the number of all three particles for an atom of Fluorine which has an
atomic mass of 19 and an atomic number of 9. It is not an ion.
2. Give the number of all three particles for an atom of Iodine which has an
atomic mass of 127 and an atomic number of 53.
3. Give the number of all three particles for Hydrogen, which has an atomic
mass of 1 and an atomic number of 1.
4. Give the number of all three particles for gold, which has an atomic mass
of 197 and an atomic number of 79.
Name: ____________________________________
(1 of 2)
Math Set # 14 Ions and Isotopes
When an atom loses or gains one or more electron it is called an “ion” and the atom
now has a charge.
For example, if a hydrogen atom has one proton (+) and one electron (-) the two
charges cancel each other out. When the electron is lost the hydrogen atom is only a
single proton (+)! This makes the whole atom have a charge of +1.
Find the charge of each ion described in the problems.
EXAMPLE: An atom loses two electrons. What is the total charge of the electrons
that were lost? What is the resulting charge of the ion?
ANSWER:
Two electrons have a total charge of -2.
The atom used to be neutral but lost negative charges so it is now
positive. Since it lost two negative particles the total charge is +2.
EXAMPLE #2: An atom gains two electrons. What is the total charge of the
electrons that were gained? What is the resulting charge of the ion?
ANSWER:
The two electrons have a total charge of -2.
The atom used to be neutral but gained negative charges so it is now
negative. Since it gained two negative particles the total charge is -2.
1. An atom loses one electron.
Total charge of the electrons that moved = _____________________
Charge of the remaining ion = ___________________________
2. An atom loses three electrons.
Total charge of the electrons that moved = __________________________
Charge of the remaining ion = ___________________________
3. An atom gains one electron.
Total charge of the electrons that moved = ________________________
Charge of the remaining ion = ____________________________
4. An atom gains three electrons.
Total charge of the electrons that moved = _________________________
Charge of the remaining ion = ______________________________
Name: ____________________________________
(2 of 2)
Math Set # 14 Ions and Isotopes
The number of protons is ALWAYS the same for an atom of a specific element.
Germanium ALWAYS has 32 protons. If you add a proton it is no longer Germanium
but becomes Arsenic. The number of neutrons, however, is NOT always the same
for an atom of Germanium. Sometimes there are 40 neutrons, but other times there
are 41. This means that a specific atom might have a slightly different atomic mass.
Method for Finding the AVERAGE atomic mass
Chlorine -35 makes up 76% of all chlorine in nature. This means that if you could
select 100 atoms of chlorine randomly 76 of them would have an atomic mass of 35.
The other 24 atoms of chlorine would be Chlorine-37 which has an atomic mass of
37. What is the average atomic mass for chlorine?
STEP ONE: Multiply the mass by the percent and divide by 100
Chlorine-35 35 amu x 76/100 = 26.60 amu (“atomic mass units”)
Chlorine-37 37 amu x 24/100 = 8.88 amu
STEP TWO: Add the amounts together. The answer is the average atomic mass
26.60 amu + 8.88 amu = 35.48 amu (NOTE: INCLUDE UNITS – amu)
DIRECTIONS: Calculate the average atomic mass for each element. Include units!
1. Boron which occurs as 20% Boron-10 and 80% Boron-11.
2. Rubidium which occurs as 72% rubidium-85 and 28% rubidium-87
3.Gallium which occurs as 60% gallium-69 and 40% gallium-71
4. Silver which occurs as 52% silver-107 and 48% silver-109
5. Silicon which occurs as 92% silicon-28, 5% silicon-29, and 3% silicon-30
Name: ___________________________________
(p. 1 of 2)
Math Set #15 Concentration
Concentration = grams of solute
milliliters of solute
Example:
What is the concentration of a solution that has 35 g of salt dissolved in
175 mL of water?
Concentration = ?
Solute = 35 g
Solvent = 175 mL
Concentration = grams of solute
milliliters of solute
Concentration = 35 g____ = 0.2 g/mL
175 mL
FOR FULL CREDIT: SET UP THE PROBLEM EXACTLY LIKE THE EXAMPLE
1. What is the concentration of solution A if it has 55 g of sugar dissolved in 500
mL of water?
2. What is the concentration of solution B if it as 36 g of sugar dissolved in 144
mL water?
3. How many grams of sugar must be dissolved in 50 mL of water to make a
concentration equal to that of solution A? How many grams of sugar must be
dissolved in 100 mL of water to make a concentration equal to that of B?
Name: ___________________________________
(p.2 of 2)
Math Set #15 Compound Percentages
Total Percentage of Elements in a compound = 100%
Example:
Propanol contains 60.0% carbon and 26.6% oxygen. Hydrogen is the
only other element in propanol. Hydrogen makes up what percentage
of the compound?
%carbon + %oxygen +%hydrogen = 100%
60.0%
+ 26.6%
+ %hydrogen = 100%
86.6% + %hydrogen = 100%
% hydrogen = 100% - 86.6%
%hydrogen = 13.4%
SHOW ALL STEPS FOR FULL CREDIT
1. Sodium Carbonate is made up of sodium, carbon, and oxygen. It has a
chemical composition of 43.4% sodium and 11.32% carbon. What is the
percentage of oxygen in this compound?
2. Sulfuric Acid is composed of hydrogen, sulfur, and oxygen. It has a percent
composition of 2.06% hydrogen and 65.3% oxygen. What is the percentage
of sulfur in this compound?
Name: ___________________________________
(p.1 of 2)
Math Set #16 Solubility
Use the following graph to answer the questions on this page and on the next page.
1. On a solubility curve, the lines
indicate the concentration of
a ____________________________
solution.
2. Values on the graph
_____________________________
(below or above)
a curve represent
unsaturated solutions
because more solute could be
dissolved at that
temperature.
3. A solution contains 70g of
NaNO3 at 30 degrees C. Is it
saturated or unsaturated?
4. A solution contains 50g of
NH4Cl at 50 degrees C. Is it
saturated or unsaturated?
5. A solution contains 20g of KCLO3 at 50 degrees C. Is it saturated or unsaturated?
6. A solution contains 70g of KI at 0 degrees. Is it saturated or unsaturated?
7. Normally solubility increases with temperature. Is that true for all the chemicals
on this graph? If not, which chemicals are the exeptions?
Name: ___________________________________
(p.2 of 2)
Math Set #16 Solubility
Use the graph on the previous page to answer the following questions.
8. What mass of solute will dissolve in 100 mL of water at the following
temperatures:
a. KNO3 at 70 degrees C _______________________________
b. NaCl at 100 degrees C ________________________________
c. NH4Cl at 90 degrees C ________________________________
9. Which substance is the most soluble in water at 15 degrees C?
10. a. What is the solubility of KCl at 5C? _______
b. What is the solubility of KCl at 25C? _______
c. What is the solubility of Ce2(SO4)3 at 10C? _______
d. What is the solubility of Ce2(SO4)3 at 50C? _______
11. a. At 90C, you dissolved 10 g of KCl in 100. g of water. Is this solution
saturated or unsaturated?
b. How do you know?
12. A mass of 100 g of NaNO3 is dissolved in 100 g of water at 80ºC.
a) Is the solution saturated or unsaturated?______________________________
b) As the solution is cooled, at what temperature should solid first appear in
the solution?
13. Use the graph to answer the following two questions:
Which compound is most soluble at 20 ºC? ________
Which is the least soluble at 40 ºC? ________
14. Which substance on the graph is least soluble at 10C? __________
Name: ____________________________________
(1 of 2)
Math Set # 17 Periodic Table
Use a Periodic table to find the information asked for below:
1.What is the atomic number of:
Calcium __________ Iron ______________ Gold ______________ Uranium _______________
2. What is the Atomic mass of:
Oxygen _____________ Silver _______________ Iron _______________ Xenon _______________
5. Does mercury have more protons and electrons than tin?
6. Is mercury a heavier element than tin?
7. Does potassium have more electrons than neon?
8. Does hydrogen have more electrons than Uranium?
9. Which has more protons, sulfur or iodine?
10. Which has more protons, iodine or silver?
11. Determine how many electrons, protons, and neutrons there are in each atom:
Argon: protons _______________
Carbon: protons ______________
Neutrons ______________
neutrons _____________
Electrons _____________
electrons _____________
DIRECTIONS: use the periodic table to locate the name for each element
12. This element uses the symbol Bi
13 This element has 47 protons
14. This element is in group 17 and has an average atomic mass of 19.
15. This element is in the lanthanides and starts with the letter Y.
16. This element has 2 protons.
17. This element is in period 6 and is abbreviated with only one letter.
Name: ____________________________________
(2 of 2)
Math Set # 17 Periodic Table
There was a newly discovered element name Johnsonium. It is to be added to the
Periodic Table of Elements on page 339 of the textbook. Johnsonium has 117
protons and 182 neutrons. It is solid at room temperature.
DIRECTIONS: Make a periodic square for this element using the key for the periodic
table on page 338 of your textbook. Make sure the color of the letters and the color
of the square are correct. Label the square with the group number and the period
number. You can give it any initials you like as long as they are not already taken.
Make another square with your own created and named element. Follow the
directions above to show how your element would fit into the periodic table.
Name: ____________________________________
(1 of 1)
Math Set #18 Periodic Table
Directions: Use the blank periodic table worksheet to complete ALL steps below.
1. Number the groups.
2. Number the periods
3. Draw a heavy lack line between the metals and nonmetals.
4. Over Group 1 write the words “alkali metals”
5. Over Group 2 write the words “alkaline earth metal”
6. Over Groups 3-12 (collectively) write “transition metals”
7. Over Group 16 write “chalcogens”
8. Over Group 17 write “halogens”
9. Over Group 18 write“Noble gases”
10. Write the names of the two rows at the bottom of the chart: lanthanides and
actinides
11. Write the symbol of each element that exists as a gas at ordinary conditions in
RED.
12. Write the symbol of each element that is a solid at ordinary conditions in
BLACK.
13. Write the symbol of each element that is a liquid at ordinary condition in BLUE.
14. Circle the symbol of each element that is a man-made.
15. Place the atomic number for each element above the symbol.
16. Use the following to color the periodic table.
Halogen
blue
Noble gases yellow
Alkali metals purple
Alkaline earth metals red
Transition elements green
Chalcogens brown
Lanthanides orange
Actinides light blue
Name: ____________________________________
(1 of 2)
Math Set # 19 Valence Electrons
Remember: Two electrons are in the first orbital, 8 in the second, and 8 in the third.
The number of electrons in the outermost orbital is the valence number.
DIRECTIONS:
1. Place the electrons in the correct orbitals for an atom of each element.
2. Write the number of valence electrons to the right of the diagram.
Hydrogen
Fluorine
Oxygen
Sulfur
Helium
Argon
Magnesium
Sodium
Boron
Carbon
Nitrogen
Aluminum
Name: ____________________________________
(2 of 2)
Math Set # 19 Valence Electrons
What is the largest number of electrons that can be in the outermost orbital of the
period 2 and period 3 elements? _________________________________
What is the largest number of electrons that can be in the outermost orbital of the
period 1 elements (Hydrogen and Helium)? _____________________________
DIRECTIONS: For each of the following elements give the valence number, circle if
the atom would fill or empty the orbital, how many electrons the atom would gain
or lose, and the resulting charge. REMEMBER, a valence of 3 or less will empty the
outermost orbital and a valence of 5 or more will gain electrons to fill the outermost
orbital. The first one is done for you
1. Sulfur:
valence = 6
for a full/empty orbital
gain 2
charge = -2 .
2. Magnesium: valence = _____ for a full/empty orbital ________________charge = _______
3. Lithium:
valence = _____ for a full/empty orbital __________________charge= _______
4. Chlorine: valence = _____ for a full/empty orbital __________________charge= _______
5. Oxygen
valence = _____ for a full/empty orbital __________________charge= _______
6. Sodium:
valence = _____ for a full/empty orbital __________________charge= _______
7. Aluminum: valence = _____ for a full/empty orbital __________________charge= _______
8. Beryllium: valence = _____ for a full/empty orbital __________________charge= _______
9. Neon:
10. Helium:
valence = _____ for a full/empty orbital __________________charge= _______
valence = _____ for a full/empty orbital __________________charge= _______
11. Flourine: valence = _____ for a full/empty orbital __________________charge= ______
12. Boron:
valence = _____ for a full/empty orbital __________________charge= _______
13. Hydrogen: valence = _____ for a full/empty orbital __________________charge= ______
14. Nitrogen: valence = _____ for a full/empty orbital __________________charge= _______
Name: ____________________________________
(1 of 3)
Math Set # 20 Lewis Structures and Ionic Bonds
REMEMBER:
An ionic bond is created between metals and nonmetals. This is because a metal in
group 1 or 2 gives up electrons easily and nonmetals in groups 16 through 18 accept
electrons easily. An ionic bond results in two or more ions being attracted to each
other. The total charge of the molecule must be zero.
Directions: For each combination of atoms indicate how many electrons are
passed from one atom to the other, the ions created, and the molecular formula.
EXAMPLE: Hydrogen and Chlorine
What will happen to the electrons? Hydrogen will give an electron to Chlorine
The resulting ions? H+ ClThe formula for this compound: HCl
1. Sodium and Chlorine
What will happen to the electrons?
The resulting ions?
The formula?
2. Magnesium and Oxygen
What will happen to the electrons?
The resulting ions?
The formula?
3. Beryllium and Sulfur
What will happen to the electrons?
The resulting ions?
The formula?
4. Hydrogen and Fluorine
What will happen to the electrons?
The resulting ions?
The formula?
5. Lithium and Chlorine
What will happen to the electrons?
The resulting ions?
The formula?
Name: ____________________________________
(2 of 3)
Math Set # 20 Lewis Structures and Ionic Bonds
Lewis Structures
REMEMBER: A full valence for all elements except Hydrogen and Helium and the
transition metals is 8. Hydrogen and Helium has a full valence of 2.
DIRECTIONS:
1. Write the element symbol
2. Find the number of valence electrons
3. Place one dark circle next to the symbol for each valence electron.
IMPORTANT RULE: electrons are added one to each side of the symbol until all the
sides have a single electron. Additional electrons make pairs on each side.
Examples:
C
Se
Xe
H
Draw Lewis Structures for the Atoms.
1. Calcium
7. Nitrogen
13. Thallium
2. Chlorine
8. Magnesium
14. Sulfur
3. Carbon
9. Hydrogen
15. Arsenic
4. Neon
10. Lithium
16. Fluorine
5. Oxygen
11. Lead
17. Radon
6. Sodium
12. Iodine
18. Aluminum
Name: ____________________________________
(3 of 3)
Math Set # 20 Lewis Structures and Ionic Bonds
+
EXAMPLES: Hydrogen and Iodine
Hydrogen will give one electron to Iodine.
Hydrogen with have a + charge
Iodine will have – charge.
H
I
DIRECTIONS: Draw the Lewis Structure for the following molecules. Use one color
for the symbol and electrons coming from the first atom and another color for the
symbol and electrons coming from the second atom. Make each diagram look like
the example.
1. Sodium and Chlorine
2. Magnesium and Oxygen
3. Beryllium and Sulfur
4. Hydrogen and Fluorine
5. Lithium and Chlorine
-
Name: ____________________________________
(1 of 4)
Math Set # 21 Naming Molecules with Ionic Bonds
REMEMBER: An ionic bond is always between a metal (left side of the periodic
table) and a nonmetal (right side of the periodic table)
Rules for IONIC molecules
1. Always name elements from left to right on the periodic table
(the positive ion goes first)
2. name the positive element without changing anything.
3. Name the negative element but change the end to an “ide”
(NOTE: You do not do anything with prefixes for ionic molecules.)
You can think of this as: ELEMENT ELEMENT”ide”
EXAMPLE:
Chlorine and Hydrogen
Name: Hydrogen Chloride
DIRECTIONS: Give the names for the following molecules:
1. Magnesium and Chlorine
________________________________________________
2. Bromine and Rubidium
________________________________________________
3. Hydrogen and Suflur
________________________________________________
4. Lithium and Oxygen
________________________________________________
5. Selenium and Calcium
________________________________________________
6. Radium and Astatine
________________________________________________
7. Potassium and Polonium
________________________________________________
8. Chloride and Potassium
________________________________________________
9. Lithium and Phosphorous ________________________________________________
10. Iodine and Sodium
________________________________________________
Name: ____________________________________
(2 of 4)
Math Set # 21 Naming Molecules with Covalent Bonds
REMEMBER: A covalent bond is always between molecules that are both on the
right side of the periodic table.
Rules for COVALENT molecules
1.
2.
3.
4.
5.
Always name elements from left to right on the periodic table
Always name elements from top to bottom on the periodic table
name the first element without changing anything.
Name the last element but change the end to an “ide”
Add prefixes to show the number of each atom in the molecule
The ONLY time there is not a prefix in front of a name is when the very first
element has only one atom. (prefixes are on page 393 of your textbook)
EXAMPLES:
One Carbon and two Oxygen
One Carbon and One Oxygen
Two Carbon and Four Oxygen
Name: Carbon Dioxide
Name: Carbon Monoxide
Name: Dicarbon Tetraoxide
Name the following molecules:
1. Two Nitrogen and one Oxygen
_______________________________________________
2. One Carbon and four Flourine
_______________________________________________
3. Two Phosphorous and five Oxygen
_______________________________________________
4. Two Boron and six Silicon
_______________________________________________
5. One Selenium and six Fluoride
_______________________________________________
6. Two Silicon and six Bromine
_______________________________________________
7. One Sulfure and four Chlorine
________________________________________________
Give the number of atoms and the name of the elements for the following molecules:
8. iodine pentafluroide
________________________________________________________________
9. dinitrogen trioxide
________________________________________________________________
10. phosphorous triiodide ________________________________________________________________
Name: ____________________________________
Math Set # 21 Chemical Formulas
(3 of 4)
A subscript it gives the number of atoms of the element just in front of it.
A coefficient (large number in front )of the molecule gives how many molecules
there are.
EXAMPLES:
H2O has 2 Hydrogen and 1 Oxygen
5 H2O has five molecules of H20 so there are 10 Hydrogen and 5 Oxygen
7NH4 has 7 molecules of Nitrogen and 28 molecules of Hydrogen
DIRECTIONS: Give the number of each kind of atom in each formula
1.
Al2O3
_____________________________________________________________
2.
2 Al2O3
_____________________________________________________________
3.
C2H6
_____________________________________________________________
4.
3 C2H6
_____________________________________________________________
5.
Na2SO4
_____________________________________________________________
6.
5 Na2SO4
_____________________________________________________________
7.
Fe2Br3
_____________________________________________________________
8.
10 Fe2Br3
_____________________________________________________________
9.
25 Fe2Br3
_____________________________________________________________
10.
11 Mg3P2
_____________________________________________________________
Name: ____________________________________
(4 of 4)
Math Set # 21 Balancing Chemical Equations
Balancing Equations
1.
2.
3.
4.
Write the equation without any coefficients.
Calculate the number of each type of atom on the left side of the arrow.
Calculate the number of each type of atom on the right side of the arrow.
Add coefficients in front of the molecules until the left side and right side
numbers match.
IMPORTANT: You can only change coefficients. You CANNOT change subscripts.
Examples:
Balance the Equation H + O2  H2O
left 1 H, 2 O right 2 H, 1 O
I give H2O a coefficient of 2 so that the number of oxygen will match
H + O2  2 H2O
left 2 H, 2 O right 4 H, 2 O
I give H a coefficient of 4 so that the number of Hydrogen will match
4H + O2  2 H2O
left 4 H, 2 O
Balance the Equation
Fe + H2O  Fe3O4 + H2
left 1 Fe, 2 H, 1 O
I give H2O a coefficient of 4 in order to balance the oxygen
Fe + 4H2O  Fe3O4 + H2
left 1 Fe, 8 H, 4 O
I give the Fe a coefficient of 3 in order to balance the iron
right 4H, 2 O
right 3 Fe, 2 H, 4 O
right 3 Fe, 2 H, 4 O
3Fe + 4H2O  Fe3O4 + H2
left
3 Fe, 8 H, 4 O
right 3 Fe, 2 H, 4 O
Everything matches except of the hydrogen. To fix this I give H2 a coefficient of 4.
3Fe + 4H2O  Fe3O4 + 4H2
left
3 Fe, 8 H, 4 O
DIRECTIONS: Balance the following Equations:
1. H2 + Cl2  HCl
2. Mg + O2  MgO
right 3 Fe, 8 H, 4 O
Name: ____________________________________
Math Set # 22 Balancing Chemical Equations
DIRECTIONS: Balance the following Equations:
1. KI + Br2  KBr + I2
2. H2 + Cl2  HCl
3. S8 + O2  SO
4. Fe2O3 + C  Fe + CO2
5. Sb + I2  SbI3
6. KBr + Cl2  Br2 + KCl
7. C3H8 + O2  3 CO2 + 4H2O
8. CHALLENGE: C6H14 + O2  H2O + CO2
(1 of 3)
Name: ____________________________________
Math Set # 22 Identifying Reaction Types
(2 of 3)
REACTION TYPES:
Synthesis: Two or more reactants combine to make a single product
Example: 2 Na + Cl2  2 NaCl
Decomposition: A single reactant breaks down to make two or more products
Example: H2CO3  H2O + CO2
Single-Displacement: An element replaces another element that is part of a
compound
Example: Zn + 2HCl  ZnCl2 + H2
Double-Displacement: An element in one compound changes places with an
element in another compound
Example: NaCl + AgF  NaF + AgCl
Combustion Reaction: A carbon compound plus O2 produces heat, CO2 and H2O.
Example: CH3OH + O2  CO2 + 2H2O
(Hint: look for O2 on one side and H2O on the other)
DIRECTIONS: Label each reaction with the reaction type:
1. H2 + Cl2  2HCl
2. 2Mg + O2  2 MgO
3. 2C2H6 + 7O2  4 CO2 + 6H2O
4. H2CO3  CO2 + H2O
5. CH4 + 2O2  CO2 + 2H2O
6. AgNO3 + KCl  AgCl + KNO3
7. 2KClO3  2KCl + 3 O2
8. Zn + HCl  ZnCl2 + H2
9. 2KCl + Na2CO3  K2CO3 + 2NaCl
10. 2H2O  2H2 + O2
Name: ____________________________________
(3 of 3)
Math Set # 22 Activation Energy
1.
1.
Answer the following questions based on the potential energy diagram shown here:
a.
Does the graph represent an endothermic
or exothermic reaction?
b.
Label the position of the reactants,
products, and activated complex.
c.
How much energy is released or
absorbed during the reaction?
d.
How much energy is required for this reaction to occur?
Answer the following questions based on the potential energy diagram shown here:
a.
Does the graph represent an endothermic
or exothermic reaction?
b.
Label the position of the reactants,
products, and activated complex.
c.
d.
How much energy is released or
absorbed during the reaction?
e.
How much energy is required for this
reaction to occur?