Formulas For The Following Compounds: Compound Copper (II) Chloride Iron
LU 1 - Tutorial
1. Write the formulas for the following compounds: Compound Copper (II) chloride Iron(II) sulphate Sodium sulphate Ammonium nitrate Sodium nitrite Potassium sulphate Magnesium phosphate Formula Compound Lithium acetate Manganese (IV) nitrate Potassium permanganate Iron (III) oxide Potassium sulphite Potassium hydrogen carbonate Sodium iodate Formula
2. Express the following numbers in scientific notation: a) 0.000000027 b) 356 c) 47 764 d) 0.096 3. Express the following numbers as decimals: a) 1.52 10-2 b) 7.78 10-8 4. Express the answers to the following calculations in scientific notation: a) 145.75 + (2.3 10-1) b) 79 500 / (2.5 102) 5. State the number of significant figure in each of the following numbers. a) …show more content…
2.0560 b) 0.000372 c) 300.6 d) 70030 6. What is the number of significant figures in each of the following measurements? a) 56 mL b) 2900 g c) 40.2 g/cm3 d) 0.0000003 cm e) 4.6 x 1019 atoms 7. Calculate and round the answers to the correct number of significant figures. (a) (b) (c) (d) (e) (f) 3.476 + 0.002 81.4 g 0.112 g 81.4 104.2 4.003 18.3 0.321 + 0.0041 1.2 6.810 0.0230 3.21
8. Calculate and round the answers to the correct number of significant figures. (a) (82.7 143) + (274 0.06) (b) (8.3 106 km) (4.13 107 km) (5.411 1012 km) (c) [(3.125 106) + (5.127 105)] (6.72 108) 9. A student experimentally determines the specific heat of water to be 4.29 J/g /oC. He then looks up the specific heat of water on a reference table and finds that is is 4.18 J/g/oC. What is his absolute error and percent error?
10.
A student takes an object with an accepted mass of 200.00 grams and masses it on his own balance. He records the mass of the object as 196.5 g. What is his percent error? 11. Carry out the following conversion of units: a) 275 cm3 to dm3 b) 750 ml to litre c) 25C to K d) 60 km hr1 to m s1 12. An average adult has 5.2 L of blood. What is the volume of blood in m3? 13. The density of silver is 1.05 104 kg/ m3. Convert the density to units of g/cm3. 14. Aluminum is a lightweight metal (density = 2.70 g/cm3) used in aircraft construction, high voltage transmission lines, beverage cans, and foils. What is its density in kg/m3? 15. The density of ammonia gas under certain conditions is 0.625 g/L. Calculate the density in g/cm3. 16. The standard enthalpy change for the combustion of hydrogen gas is -286 kJ per mole of hydrogen. How much heat is released when 1.000 litres of hydrogen gas at STP is burned? (at STP, the volume of 1 mol of any ideal gas is 22.414 liters) 17. The human body is 0.0040% iron. How many milligrams of iron does a 64 kg person contain? 18. How many H atoms are present in 23.6 g of urea (NH2)2CO, which is used as fertilizers? Given 1 mol of urea has a mass of 60.06 g. 19. Complete the table for some of the elements occurring naturally. Element Sodium Scandium Arsenic Gold Symbol Na Sc As Au 21 79 Proton number Nucleon number 23 Number of neutrons 12 24 42 118 79 Number of …show more content…
electrons
20. Complete the table for some of the elements occurring naturally. Element Beryllium Oxygen Potassium Copper Symbol of Element Be O K Cu 19 29
40 18 X
Proton number 4
Nucleon number
Number of neutrons 5
Number of electrons 8
Symbolic representation
16 39 64 isotope.
20
19 27
21. P+ and Q are isoelectronic with a) b) c)
State the nucleon number of the isotope X State the number of protons in P and Q Identity the element P and Q
22. Do you agree with the statements below? If yes, mark () and if no, mark () No. Statement a. b. c. d. e. f. g. Any element can have only 2 isotopes 2 isotopes of an element may not have the same proton number Most elements do not have isotopes Isoelectronic particles must have the same number of electrons. Isoelectronic particles must have the same number of protons also. An atom X receives 2 electrons, then it is represented in symbol as X2An atom W loses 4 electrons, then it is represented in symbol as W4+ Answer
23. (Challenging) When a neutron is added to the nucleus of an atom: a) the proton number is altered b) the nucleon number is changed c) the new atom is an isotope of the original atom 24. Calculate the relative molecular mass of the following compounds: a) b) c) d) HNO3 Na2CO3 KClO4 Al2(SO4)3
25. The element boron consists of two isotopes,
11 5 B is
10 11 5 B and 5 B .
Their masses, based on the
10 5 B
is
carbon scale, are 10.01 and 11.01, respectively. The abundance of
20.0% and the
abundance of 80.0%. What is the atomic mass of boron? 26. In the ionization chamber of a mass spectrometer, bombardment of electrons into the gaseous particles of substance under investigation will form positive ions. If the gaseous particles are P and Q: a) write equations for the reactions b) if P is heavier than Q, which ion is deflected more by a magnetic field? c) if P is 1 H , state clearly the number of electrons, protons and neutrons after it has 1 gone through the ionization chamber.
27. A metallic element M is analyzed using a mass spectrometer. The mass spectrum is as below:
Relative abundance
40
41 m/e
42
Write three conclusions based on the mass spectrum. 28. If isotopes of chlorine are 35Cl and 37Cl, write down the types of chemical species that will be formed in a chlorine gas (Cl2) 29. If isotopes of chlorine are 35Cl and 37Cl, write down the types of chemical species that may be formed in the ionization chamber of a mass spectrometer. 30. Gas CO is analyzed. If carbon has isotopes of 12C and 14C and that of oxygen are 16O and 17 O, write down the types of singly charged ions that can be detected by the mass spectrometer. 31. Chloromethane (CH3Cl) is analyzed using a mass spectrometer. The peaks observed gave m/e as 15, 35, 37, 50 and 52. Assuming RAM of C=12.0; H=1.0; and Cl has isotopes of 35.0 and 37.0, identify the charged particles responsible for each of the peaks.
1. Write the formulas for the following compounds: Compound Copper (II) chloride Iron(II) sulphate Sodium sulphate Ammonium nitrate Sodium nitrite Potassium sulphate Magnesium phosphate Formula Compound Lithium acetate Manganese (IV) nitrate Potassium permanganate Iron (III) oxide Potassium sulphite Potassium hydrogen carbonate Sodium iodate Formula
2. Express the following numbers in scientific notation: a) 0.000000027 b) 356 c) 47 764 d) 0.096 3. Express the following numbers as decimals: a) 1.52 10-2 b) 7.78 10-8 4. Express the answers to the following calculations in scientific notation: a) 145.75 + (2.3 10-1) b) 79 500 / (2.5 102) 5. State the number of significant figure in each of the following numbers. a) …show more content…
2.0560 b) 0.000372 c) 300.6 d) 70030 6. What is the number of significant figures in each of the following measurements? a) 56 mL b) 2900 g c) 40.2 g/cm3 d) 0.0000003 cm e) 4.6 x 1019 atoms 7. Calculate and round the answers to the correct number of significant figures. (a) (b) (c) (d) (e) (f) 3.476 + 0.002 81.4 g 0.112 g 81.4 104.2 4.003 18.3 0.321 + 0.0041 1.2 6.810 0.0230 3.21
8. Calculate and round the answers to the correct number of significant figures. (a) (82.7 143) + (274 0.06) (b) (8.3 106 km) (4.13 107 km) (5.411 1012 km) (c) [(3.125 106) + (5.127 105)] (6.72 108) 9. A student experimentally determines the specific heat of water to be 4.29 J/g /oC. He then looks up the specific heat of water on a reference table and finds that is is 4.18 J/g/oC. What is his absolute error and percent error?
10.
A student takes an object with an accepted mass of 200.00 grams and masses it on his own balance. He records the mass of the object as 196.5 g. What is his percent error? 11. Carry out the following conversion of units: a) 275 cm3 to dm3 b) 750 ml to litre c) 25C to K d) 60 km hr1 to m s1 12. An average adult has 5.2 L of blood. What is the volume of blood in m3? 13. The density of silver is 1.05 104 kg/ m3. Convert the density to units of g/cm3. 14. Aluminum is a lightweight metal (density = 2.70 g/cm3) used in aircraft construction, high voltage transmission lines, beverage cans, and foils. What is its density in kg/m3? 15. The density of ammonia gas under certain conditions is 0.625 g/L. Calculate the density in g/cm3. 16. The standard enthalpy change for the combustion of hydrogen gas is -286 kJ per mole of hydrogen. How much heat is released when 1.000 litres of hydrogen gas at STP is burned? (at STP, the volume of 1 mol of any ideal gas is 22.414 liters) 17. The human body is 0.0040% iron. How many milligrams of iron does a 64 kg person contain? 18. How many H atoms are present in 23.6 g of urea (NH2)2CO, which is used as fertilizers? Given 1 mol of urea has a mass of 60.06 g. 19. Complete the table for some of the elements occurring naturally. Element Sodium Scandium Arsenic Gold Symbol Na Sc As Au 21 79 Proton number Nucleon number 23 Number of neutrons 12 24 42 118 79 Number of …show more content…
electrons
20. Complete the table for some of the elements occurring naturally. Element Beryllium Oxygen Potassium Copper Symbol of Element Be O K Cu 19 29
40 18 X
Proton number 4
Nucleon number
Number of neutrons 5
Number of electrons 8
Symbolic representation
16 39 64 isotope.
20
19 27
21. P+ and Q are isoelectronic with a) b) c)
State the nucleon number of the isotope X State the number of protons in P and Q Identity the element P and Q
22. Do you agree with the statements below? If yes, mark () and if no, mark () No. Statement a. b. c. d. e. f. g. Any element can have only 2 isotopes 2 isotopes of an element may not have the same proton number Most elements do not have isotopes Isoelectronic particles must have the same number of electrons. Isoelectronic particles must have the same number of protons also. An atom X receives 2 electrons, then it is represented in symbol as X2An atom W loses 4 electrons, then it is represented in symbol as W4+ Answer
23. (Challenging) When a neutron is added to the nucleus of an atom: a) the proton number is altered b) the nucleon number is changed c) the new atom is an isotope of the original atom 24. Calculate the relative molecular mass of the following compounds: a) b) c) d) HNO3 Na2CO3 KClO4 Al2(SO4)3
25. The element boron consists of two isotopes,
11 5 B is
10 11 5 B and 5 B .
Their masses, based on the
10 5 B
is
carbon scale, are 10.01 and 11.01, respectively. The abundance of
20.0% and the
abundance of 80.0%. What is the atomic mass of boron? 26. In the ionization chamber of a mass spectrometer, bombardment of electrons into the gaseous particles of substance under investigation will form positive ions. If the gaseous particles are P and Q: a) write equations for the reactions b) if P is heavier than Q, which ion is deflected more by a magnetic field? c) if P is 1 H , state clearly the number of electrons, protons and neutrons after it has 1 gone through the ionization chamber.
27. A metallic element M is analyzed using a mass spectrometer. The mass spectrum is as below:
Relative abundance
40
41 m/e
42
Write three conclusions based on the mass spectrum. 28. If isotopes of chlorine are 35Cl and 37Cl, write down the types of chemical species that will be formed in a chlorine gas (Cl2) 29. If isotopes of chlorine are 35Cl and 37Cl, write down the types of chemical species that may be formed in the ionization chamber of a mass spectrometer. 30. Gas CO is analyzed. If carbon has isotopes of 12C and 14C and that of oxygen are 16O and 17 O, write down the types of singly charged ions that can be detected by the mass spectrometer. 31. Chloromethane (CH3Cl) is analyzed using a mass spectrometer. The peaks observed gave m/e as 15, 35, 37, 50 and 52. Assuming RAM of C=12.0; H=1.0; and Cl has isotopes of 35.0 and 37.0, identify the charged particles responsible for each of the peaks.