Significant Figures Worksheet
Significant Figures Worksheet Determine the number of significant figures in each of the following: (a) 5.432 g (b) 40.319 g (c) 146 cm (d) 3.285 cm (e) 0.189 s (f) 429.3 mm (g) 2873.0 A (h) 990 ml (i) 0.0000246 g (j) 1.04 x 1012 g (k) 5.59 x 10-7 m (l) 0.0000242 mg Complete the following addition/subtraction questions: 12 cm + 0.031 cm + 7969 cm = 0.085 cm + 0.062 cm + 0.14 cm = 3.419 g + 3.912 g + 7.0518 g + 0.00013 g = 30.5 g - 16.82 g + 41.07 g + 85.219 g = 143.0 cm + 289.25 cm + 68.45 cm - 6.00 cm = 3. Complete the following multiplication questions (be careful with units): (a) 2.89 cm x 4.01 cm = (b) 17.3 cm x 6.2 cm = (c) 5.08 m x 1.2 m = (d) 5.00 mm x 7.3216 mm = (e) 4.218 cm x 6.5 cm = (f) (4.8 x 102 m)(2.101 x 103 m) = Complete the following division questions (be careful with units): (a) 8.071 cm2 = (b) 24789.4 km2 = 4.216 cm 43.5 km (c) 4.819 cm2 = (d) 2.23 m2 = 9.852 cm 18.941 m Solutions: 1. a) 4 b) 5 c) 3 d) 4 e) 3 f) 4 g) 5 h) 2 i) 3 j) 3 k) 3 i) 3 2. a) 7981 cm b)0.28 cm c) 7.052 g d)140.0 g e) 494.7cm 3. a) 11.6 cm2 b)110 cm2 c) 6.1 m2 d) 36.6 mm2 e) 27 cm2 f) 1.0x106 m2 4. a) 1.914 cm b) 570 km c) 0.4891 km d) 0.118 m
Accuracy & Precision Worksheet Accuracy: refers to how close a measurement is to a true, accepted or target value. Precision: Refers to the reproducibility of a series of measurements Percent Error (Difference): (Measurement – Target Value)*100 Target Value 1. The following measurements were made to determine the density of a material whose value was, according to the Handbook of Chemistry and Physics, 1.24 g/mL Trial #1 1.20 g/mL Trial #2 1.22 g/mL Trial #3 1.22 g/mL a. make a general comment on the accuracy of these results b. make a general comment on the precision of these results c. use the average of the three trials as the “measured value” and determine the numerical value for the percent error.
Classification of Matter PART A – COMPOSITION OF MATTER Classify the following as element, compound, heterogeneous mixture, or solution (homogeneous mixture). aluminum orange juice air carbon dioxide
Compare and contrast a mixture and a compound. How are they alike? How are they different? Use complete sentences.
PART B – SOLUTIONS, COLLOIDS (FOG), PARTICLES)
AND
SUSPENSIONS (POND
WATER WITH LARGE
For each type of mixture draw a picture representing the size and distribution of particles in a liquid.
PART C – PROPERTIES & CHANGES OF MATTER Classify the following properties of matter as chemical (C) or physical (P). flexible combustible boils at 20C low reactivity with acids
Classify the following as chemical (C) or physical (P) changes. grapes fermenting copper melting recycling aluminum gasoline exploding
Worksheet: Atoms, Isotopes, and Ions Atoms The number of protons in an atom determines the identity of the atom. Atomic # = # Protons In a neutral atom, the number of positive protons equals the number of negative electrons. # Protons = # Electrons Protons and neutrons both have a mass of 1 amu. The mass of the electron is negligible compared to the mass of the proton and neutron. Thus the mass number, or the mass of the atom, is the sum of the number of protons and neutrons. Mass # = # Protons + # Neutrons
Name Selenium
Symbol
Atomic #
Mass #
# Protons
222
86
# Neutrons 46
# Electrons
118
79
11
12
Isotopes The number of neutrons in any specific type of atom can vary. Atoms of the same element with different numbers of neutrons are called isotopes. Isotopes are distinguished from each other by including the mass number with the name or symbol.
Name
Symbol 235 U
Atomic #
Mass #
# Protons
# Neutrons
# Electrons
238
U
Carbon-12 Carbon-13
Ions As we have seen, in a neutral atom, the number of protons and the number of electrons is equal. Atoms can gain or lose electrons to become ions. Ions are charged atoms resulting from the difference in number of positive protons and negative electrons. A cation is a positive ion. A cation results when an atom loses electrons. # Protons > # Electrons An anion is a negative ion. An anion results when an atom gains electrons. # Electrons > # Protons Ions are distinguished from atoms by including the ion charge as a superscript in the symbol.
Name
Symbol Al+3
Iron ion
Atomic #
Mass #
# Protons
# Neutrons 14
# Electrons
56
24 15
F-1
15
19
Grams and Particles Conversion Worksheet
18
Cation or Anion?
1) How many formula units are there in 24.0 grams of FeF3?
2) How many grams are there in 2.30 x 1024 atoms of silver?
3) How many grams are there in 7.40 x 1023 molecules of silver nitrate?
4) How many molecules are there in 200 grams carbon tetrachloride?
Moles, Molecules, and Grams Worksheet – Answer Key 1) How many molecules are there in 24.0 grams of FeF3? 1.28 x 1023 molecules 2) How many grams are there in 2.30 x 1024 atoms of silver? 421 grams 3) How many grams are there in 7.40 x 1023 molecules of silver nitrate? 209 grams 4)) How many molecules are there in 200. grams of CCl4? 7.82 x 1023 molecules
Percent Composition Percent composition is the percent by mass of each element found in a compound. Example: What percent of iron(III) hydroxide, Fe(OH)3, is oxygen? Step 1: Find the molar mass of the compound. 1 mol Fe = 55.85 g 3 mol O = 3 × 16.00 g = 48.00 g 3 mol H = 3 × 1.008 g = 3.024 g Molar Mass Fe(OH)3 = 106.87 g/mo Step 2: Find the percentage by dividing the part by the whole and multiplying by 100.
×100 % = 44.91% oxygen Solve the following. What percent of magnesium bromide, MgBr2, is magnesium?
What percent of glucose, C6H12O6, is carbon?
What percent of Zn3(PO4)2 is zinc?
What is the percent composition of water in the hydrate magnesium sulfate heptahydrate MgSO4 * 7H20
SOME Periodic Table Questions 1. What period are the following elements in?
a. He _______________
b. Ge _________________
c. Rb _______________
d. I __________________
2. What group are the following elements?
a. Sulfur _______________
b. Ca _________________
c. Iodine _______________
d. Fe _________________
3. Give me an atom with the following characteristics.
a. Halogen _________________ b. Nonmetal ________________
c. Alkali metal ______________ d. metalloid ________________
e. Lanthanide series __________
f. Alkaline Earth metal ________________
g. Transition metal ___________
h. Nobel gas ________________
4. Write the electron configuration for
a. Li _______________________________________________________________
b. Na ______________________________________________________________
c. K _______________________________________________________________
5. Write the quantum numbers for Sb 6. Provide an example of a violation of Pauli Exclusion Principle
Indicate trends across period and within groups for Atomic Radius Ionization Energy Electronegativity Increasing metallic properties Coulombic attraction Shielding Effect
DoD
Do you know patterns for valence electrons and oxidation numbers? What do you have to remember about Fe Pb Sn Cu? What do you have to remember about Zn and Ag? When is there the greatest increase in Successive Ionization energy?
Why do electron affinity values have negative numbers?
Bond Polarity 1. What one requirement must be met for a single bond to be polar?
2. Which atom of the following is most electronegative? a. Li b. Ge c. Br
3. Which atom of the following is least electronegative? a. As b. Se c. S
4. Determine if each of the following bonds is polar or nonpolar: a. Se-Cl b. Al-Cl c. I-F
d. Cl-Cl
5. List the following bonds in order of increasing polarity: a. N-O b. F-O c. O-O d. S-O
6. Which of the following is the correct Lewis dot structure for carbon dioxide?
Nomenclature Practice For each of the following questions, determine whether the compound is ionic or covalent and name it appropriately. 1) Na2CO3 _________________________________________ 2) P2O5 _________________________________________ 3) I2 _________________________________________ 4) FeSO4 _________________________________________ 5) SiO2 _________________________________________ 6) GaCl3 _________________________________________ 7) CoBr2 _________________________________________ 8) B2H4 _________________________________________ 9) CO _________________________________________ 10) P4 _________________________________________
For each of the following questions, determine whether the compound is ionic or covalent and write the appropriate formula for it. 11) dinitrogen trioxide _________________________________________ 12) nitrogen _________________________________________ 13) methane _________________________________________
14) lithium acetate _________________________________________ 15) phosphorus trifluoride _________________________________________ 16) vanadium (V) oxide _________________________________________ 17) aluminum hydroxide _________________________________________ 18) zinc sulfide _________________________________________ 19) silicon tetrafluoride _________________________________________ 20) silver (I) phosphate _________________________________________
Nomenclature Practice Solutions For each of the following questions, determine whether the compound is ionic or covalent and name it appropriately. 1) Na2CO3 sodium carbonate 2) P2O5 diphosphorus pentoxide 3) I2 Iodide 4) FeSO4 iron (II) sulfate 5) SiO2 silicon dioxide 6) GaCl3 gallium chloride 7) CoBr2 cobalt (II) bromide
8) B2H4 diboron tetrahydride 9) CO carbon monoxide 10) P4 phosphorus
For each of the following questions, determine whether the compound is ionic or covalent and write the appropriate formula for it. 11) dinitrogen trioxide N2O3 12) nitrogen N2 13) carbon tetrahydride or methane CH4 14) lithium acetate LiC2H3O2 15) phosphorus trifluoride PF3 16) vanadium (V) oxide V2O5 17) aluminum hydroxide Al(OH)3 18) zinc sulfide ZnS 19) silicon tetrafluoride SiF4 20) silver phosphate Ag3PO4
Accuracy & Precision Worksheet Accuracy: refers to how close a measurement is to a true, accepted or target value. Precision: Refers to the reproducibility of a series of measurements Percent Error (Difference): (Measurement – Target Value)*100 Target Value 1. The following measurements were made to determine the density of a material whose value was, according to the Handbook of Chemistry and Physics, 1.24 g/mL Trial #1 1.20 g/mL Trial #2 1.22 g/mL Trial #3 1.22 g/mL a. make a general comment on the accuracy of these results b. make a general comment on the precision of these results c. use the average of the three trials as the “measured value” and determine the numerical value for the percent error.
Classification of Matter PART A – COMPOSITION OF MATTER Classify the following as element, compound, heterogeneous mixture, or solution (homogeneous mixture). aluminum orange juice air carbon dioxide
Compare and contrast a mixture and a compound. How are they alike? How are they different? Use complete sentences.
PART B – SOLUTIONS, COLLOIDS (FOG), PARTICLES)
AND
SUSPENSIONS (POND
WATER WITH LARGE
For each type of mixture draw a picture representing the size and distribution of particles in a liquid.
PART C – PROPERTIES & CHANGES OF MATTER Classify the following properties of matter as chemical (C) or physical (P). flexible combustible boils at 20C low reactivity with acids
Classify the following as chemical (C) or physical (P) changes. grapes fermenting copper melting recycling aluminum gasoline exploding
Worksheet: Atoms, Isotopes, and Ions Atoms The number of protons in an atom determines the identity of the atom. Atomic # = # Protons In a neutral atom, the number of positive protons equals the number of negative electrons. # Protons = # Electrons Protons and neutrons both have a mass of 1 amu. The mass of the electron is negligible compared to the mass of the proton and neutron. Thus the mass number, or the mass of the atom, is the sum of the number of protons and neutrons. Mass # = # Protons + # Neutrons
Name Selenium
Symbol
Atomic #
Mass #
# Protons
222
86
# Neutrons 46
# Electrons
118
79
11
12
Isotopes The number of neutrons in any specific type of atom can vary. Atoms of the same element with different numbers of neutrons are called isotopes. Isotopes are distinguished from each other by including the mass number with the name or symbol.
Name
Symbol 235 U
Atomic #
Mass #
# Protons
# Neutrons
# Electrons
238
U
Carbon-12 Carbon-13
Ions As we have seen, in a neutral atom, the number of protons and the number of electrons is equal. Atoms can gain or lose electrons to become ions. Ions are charged atoms resulting from the difference in number of positive protons and negative electrons. A cation is a positive ion. A cation results when an atom loses electrons. # Protons > # Electrons An anion is a negative ion. An anion results when an atom gains electrons. # Electrons > # Protons Ions are distinguished from atoms by including the ion charge as a superscript in the symbol.
Name
Symbol Al+3
Iron ion
Atomic #
Mass #
# Protons
# Neutrons 14
# Electrons
56
24 15
F-1
15
19
Grams and Particles Conversion Worksheet
18
Cation or Anion?
1) How many formula units are there in 24.0 grams of FeF3?
2) How many grams are there in 2.30 x 1024 atoms of silver?
3) How many grams are there in 7.40 x 1023 molecules of silver nitrate?
4) How many molecules are there in 200 grams carbon tetrachloride?
Moles, Molecules, and Grams Worksheet – Answer Key 1) How many molecules are there in 24.0 grams of FeF3? 1.28 x 1023 molecules 2) How many grams are there in 2.30 x 1024 atoms of silver? 421 grams 3) How many grams are there in 7.40 x 1023 molecules of silver nitrate? 209 grams 4)) How many molecules are there in 200. grams of CCl4? 7.82 x 1023 molecules
Percent Composition Percent composition is the percent by mass of each element found in a compound. Example: What percent of iron(III) hydroxide, Fe(OH)3, is oxygen? Step 1: Find the molar mass of the compound. 1 mol Fe = 55.85 g 3 mol O = 3 × 16.00 g = 48.00 g 3 mol H = 3 × 1.008 g = 3.024 g Molar Mass Fe(OH)3 = 106.87 g/mo Step 2: Find the percentage by dividing the part by the whole and multiplying by 100.
×100 % = 44.91% oxygen Solve the following. What percent of magnesium bromide, MgBr2, is magnesium?
What percent of glucose, C6H12O6, is carbon?
What percent of Zn3(PO4)2 is zinc?
What is the percent composition of water in the hydrate magnesium sulfate heptahydrate MgSO4 * 7H20
SOME Periodic Table Questions 1. What period are the following elements in?
a. He _______________
b. Ge _________________
c. Rb _______________
d. I __________________
2. What group are the following elements?
a. Sulfur _______________
b. Ca _________________
c. Iodine _______________
d. Fe _________________
3. Give me an atom with the following characteristics.
a. Halogen _________________ b. Nonmetal ________________
c. Alkali metal ______________ d. metalloid ________________
e. Lanthanide series __________
f. Alkaline Earth metal ________________
g. Transition metal ___________
h. Nobel gas ________________
4. Write the electron configuration for
a. Li _______________________________________________________________
b. Na ______________________________________________________________
c. K _______________________________________________________________
5. Write the quantum numbers for Sb 6. Provide an example of a violation of Pauli Exclusion Principle
Indicate trends across period and within groups for Atomic Radius Ionization Energy Electronegativity Increasing metallic properties Coulombic attraction Shielding Effect
DoD
Do you know patterns for valence electrons and oxidation numbers? What do you have to remember about Fe Pb Sn Cu? What do you have to remember about Zn and Ag? When is there the greatest increase in Successive Ionization energy?
Why do electron affinity values have negative numbers?
Bond Polarity 1. What one requirement must be met for a single bond to be polar?
2. Which atom of the following is most electronegative? a. Li b. Ge c. Br
3. Which atom of the following is least electronegative? a. As b. Se c. S
4. Determine if each of the following bonds is polar or nonpolar: a. Se-Cl b. Al-Cl c. I-F
d. Cl-Cl
5. List the following bonds in order of increasing polarity: a. N-O b. F-O c. O-O d. S-O
6. Which of the following is the correct Lewis dot structure for carbon dioxide?
Nomenclature Practice For each of the following questions, determine whether the compound is ionic or covalent and name it appropriately. 1) Na2CO3 _________________________________________ 2) P2O5 _________________________________________ 3) I2 _________________________________________ 4) FeSO4 _________________________________________ 5) SiO2 _________________________________________ 6) GaCl3 _________________________________________ 7) CoBr2 _________________________________________ 8) B2H4 _________________________________________ 9) CO _________________________________________ 10) P4 _________________________________________
For each of the following questions, determine whether the compound is ionic or covalent and write the appropriate formula for it. 11) dinitrogen trioxide _________________________________________ 12) nitrogen _________________________________________ 13) methane _________________________________________
14) lithium acetate _________________________________________ 15) phosphorus trifluoride _________________________________________ 16) vanadium (V) oxide _________________________________________ 17) aluminum hydroxide _________________________________________ 18) zinc sulfide _________________________________________ 19) silicon tetrafluoride _________________________________________ 20) silver (I) phosphate _________________________________________
Nomenclature Practice Solutions For each of the following questions, determine whether the compound is ionic or covalent and name it appropriately. 1) Na2CO3 sodium carbonate 2) P2O5 diphosphorus pentoxide 3) I2 Iodide 4) FeSO4 iron (II) sulfate 5) SiO2 silicon dioxide 6) GaCl3 gallium chloride 7) CoBr2 cobalt (II) bromide
8) B2H4 diboron tetrahydride 9) CO carbon monoxide 10) P4 phosphorus
For each of the following questions, determine whether the compound is ionic or covalent and write the appropriate formula for it. 11) dinitrogen trioxide N2O3 12) nitrogen N2 13) carbon tetrahydride or methane CH4 14) lithium acetate LiC2H3O2 15) phosphorus trifluoride PF3 16) vanadium (V) oxide V2O5 17) aluminum hydroxide Al(OH)3 18) zinc sulfide ZnS 19) silicon tetrafluoride SiF4 20) silver phosphate Ag3PO4
