1. An atom is made up of protons electrons and neutrons. Describe these particle
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1. An atom is made up of protons electrons and neutrons. Describe these particles by stating their masses and charges. The masses should be stated in both grams and in amu units. Describe various atomic models noting the timeline for each model, including contributions (discovery/philosophy) made by Aristotle, Democritis, Dalton, Thompson, Rutherford, Chadwick, and Bohr. Describe at least 2 experiments that led scientists to this model of an atom. 2. Spectroscopy has many applications. What causes atoms to emit characteristic spectra? Describe atomic emission spectroscopy using the words photon, electron configurations, ground state, excited state, energy changes, wavelength and frequency. Explain how atomic emission spectra are quantized. What did (would) Isaac Newton think about the modern atomic structure? Describe what each term in the following equations represents; E = h and E = h c / What is the energy of a photon of light with a wavelength of 546 nm? What is the energy of a mole of photons with a wavelength of 546 nm? What color are the photons? 3. Electron configurations, especially valence electrons, are useful for understanding how an atom bonds with other atoms to make compounds. Explain how the periodic table is set up to make “seeing” valence electrons easier. Describe 2 other trends which the periodic table helps us see. 4. Diatomic elements, which are molecules, exist because sometimes 2 atoms would rather be combined with each other than alone. Why is this so and what are the 7 diatomic elements? 5. Define atomic radius and ionization energy. Describe how atomic size and ionization energy are related. Describe how an atom becomes an ion. Discuss why certain atoms become more stable cations, and others tend to become more stable anions, while some do not tend to form ions at all. 6. Determine the number of protons, electrons and neutrons in; -an atom of silver (Ag) with a mass of 108. -an ion of iron (Fe) with a 3+ charge and a mass of 56 - an ion of fluorine with a 1- charge and a mass of 19 7. Draw the Lewis structures for a) CO b) CO2 c) H2O d) CH4 e) H2CO3 8. The shape of a molecule and what atoms are in it determines the relative polarity of a molecule. Explain the term electronegativity. Explain why water is considered to be very polar while methane, CH4, is considered to be non polar. 9. Ionic and Covalent bonding occur in many compounds. Describe 2 compounds that have only ionic bonds and 2 compounds that have covalent bonds only. How does the type of bonding affect the molecules properties? 10. Sulfuric acid is a key chemical to the world’s economy. Describe how the acid is manufactured showing all chemical reactions (balanced) beginning with the element that is used to make sulfuric acid. Describe 5 other products that sulfuric acid is used to make. 11. Show a balanced chemical equation for the reaction of butane and oxygen producing carbon dioxide and water. If 100 g of butane are reacted with unlimited amounts of oxygen, how much carbon dioxide (in grams) and how much water (in grams) should form? 12. Oxidation-reduction (REDOX) is a term used to describe many reactions. When sodium, a metal, is placed in water a violent reaction can occur. This produces hydrogen gas and sodium hydroxide. Show a balanced equation for this reaction. During this reaction is the sodium oxidized or reduced? 13. Nitric oxide (nitrogen monoxide), NO, is a small molecule that at ordinary temps and pressures is a gas. The gas is part of smog and also has recently been found in humans. The molecule has a Lewis structure which violates the octet rule. Draw the structure of the molecule and describe how it violates the octet rule. Show with equations how NO is created and becomes smog. Discuss (or show with equations) how NO is formed in the human body and what effects is has. 1. An atom is made up of protons electrons and neutrons. Describe these particles by stating their masses and charges. The masses should be stated in both grams and in amu units. Describe various atomic models noting the timeline for each model, including contributions (discovery/philosophy) made by Aristotle, Democritis, Dalton, Thompson, Rutherford, Chadwick, and Bohr. Describe at least 2 experiments that led scientists to this model of an atom. 2. Spectroscopy has many applications. What causes atoms to emit characteristic spectra? Describe atomic emission spectroscopy using the words photon, electron configurations, ground state, excited state, energy changes, wavelength and frequency. Explain how atomic emission spectra are quantized. What did (would) Isaac Newton think about the modern atomic structure? Describe what each term in the following equations represents; E = h and E = h c / What is the energy of a photon of light with a wavelength of 546 nm? What is the energy of a mole of photons with a wavelength of 546 nm? What color are the photons? 3. Electron configurations, especially valence electrons, are useful for understanding how an atom bonds with other atoms to make compounds. Explain how the periodic table is set up to make “seeing” valence electrons easier. Describe 2 other trends which the periodic table helps us see. 4. Diatomic elements, which are molecules, exist because sometimes 2 atoms would rather be combined with each other than alone. Why is this so and what are the 7 diatomic elements? 5. Define atomic radius and ionization energy. Describe how atomic size and ionization energy are related. Describe how an atom becomes an ion. Discuss why certain atoms become more stable cations, and others tend to become more stable anions, while some do not tend to form ions at all. 6. Determine the number of protons, electrons and neutrons in; -an atom of silver (Ag) with a mass of 108. -an ion of iron (Fe) with a 3+ charge and a mass of 56 - an ion of fluorine with a 1- charge and a mass of 19 7. Draw the Lewis structures for a) CO b) CO2 c) H2O d) CH4 e) H2CO3 8. The shape of a molecule and what atoms are in it determines the relative polarity of a molecule. Explain the term electronegativity. Explain why water is considered to be very polar while methane, CH4, is considered to be non polar. 9. Ionic and Covalent bonding occur in many compounds. Describe 2 compounds that have only ionic bonds and 2 compounds that have covalent bonds only. How does the type of bonding affect the molecules properties? 10. Sulfuric acid is a key chemical to the world’s economy. Describe how the acid is manufactured showing all chemical reactions (balanced) beginning with the element that is used to make sulfuric acid. Describe 5 other products that sulfuric acid is used to make. 11. Show a balanced chemical equation for the reaction of butane and oxygen producing carbon dioxide and water. If 100 g of butane are reacted with unlimited amounts of oxygen, how much carbon dioxide (in grams) and how much water (in grams) should form? 12. Oxidation-reduction (REDOX) is a term used to describe many reactions. When sodium, a metal, is placed in water a violent reaction can occur. This produces hydrogen gas and sodium hydroxide. Show a balanced equation for this reaction. During this reaction is the sodium oxidized or reduced? 13. Nitric oxide (nitrogen monoxide), NO, is a small molecule that at ordinary temps and pressures is a gas. The gas is part of smog and also has recently been found in humans. The molecule has a Lewis structure which violates the octet rule. Draw the structure of the molecule and describe how it violates the octet rule. Show with equations how NO is created and becomes smog. Discuss (or show with equations) how NO is formed in the human body and what effects is has. 1. An atom is made up of protons electrons and neutrons. Describe these particles by stating their masses and charges. The masses should be stated in both grams and in amu units. Describe various atomic models noting the timeline for each model, including contributions (discovery/philosophy) made by Aristotle, Democritis, Dalton, Thompson, Rutherford, Chadwick, and Bohr. Describe at least 2 experiments that led scientists to this model of an atom. 2. Spectroscopy has many applications. What causes atoms to emit characteristic spectra? Describe atomic emission spectroscopy using the words photon, electron configurations, ground state, excited state, energy changes, wavelength and frequency. Explain how atomic emission spectra are quantized. What did (would) Isaac Newton think about the modern atomic structure? Describe what each term in the following equations represents; E = h and E = h c / What is the energy of a photon of light with a wavelength of 546 nm? What is the energy of a mole of photons with a wavelength of 546 nm? What color are the photons? 3. Electron configurations, especially valence electrons, are useful for understanding how an atom bonds with other atoms to make compounds. Explain how the periodic table is set up to make “seeing” valence electrons easier. Describe 2 other trends which the periodic table helps us see. 4. Diatomic elements, which are molecules, exist because sometimes 2 atoms would rather be combined with each other than alone. Why is this so and what are the 7 diatomic elements? 5. Define atomic radius and ionization energy. Describe how atomic size and ionization energy are related. Describe how an atom becomes an ion. Discuss why certain atoms become more stable cations, and others tend to become more stable anions, while some do not tend to form ions at all. 6. Determine the number of protons, electrons and neutrons in; -an atom of silver (Ag) with a mass of 108. -an ion of iron (Fe) with a 3+ charge and a mass of 56 - an ion of fluorine with a 1- charge and a mass of 19 7. Draw the Lewis structures for a) CO b) CO2 c) H2O d) CH4 e) H2CO3 8. The shape of a molecule and what atoms are in it determines the relative polarity of a molecule. Explain the term electronegativity. Explain why water is considered to be very polar while methane, CH4, is considered to be non polar. 9. Ionic and Covalent bonding occur in many compounds. Describe 2 compounds that have only ionic bonds and 2 compounds that have covalent bonds only. How does the type of bonding affect the molecules properties? 10. Sulfuric acid is a key chemical to the world’s economy. Describe how the acid is manufactured showing all chemical reactions (balanced) beginning with the element that is used to make sulfuric acid. Describe 5 other products that sulfuric acid is used to make. 11. Show a balanced chemical equation for the reaction of butane and oxygen producing carbon dioxide and water. If 100 g of butane are reacted with unlimited amounts of oxygen, how much carbon dioxide (in grams) and how much water (in grams) should form? 12. Oxidation-reduction (REDOX) is a term used to describe many reactions. When sodium, a metal, is placed in water a violent reaction can occur. This produces hydrogen gas and sodium hydroxide. Show a balanced equation for this reaction. During this reaction is the sodium oxidized or reduced? 13. Nitric oxide (nitrogen monoxide), NO, is a small molecule that at ordinary temps and pressures is a gas. The gas is part of smog and also has recently been found in humans. The molecule has a Lewis structure which violates the octet rule. Draw the structure of the molecule and describe how it violates the octet rule. Show with equations how NO is created and becomes smog. Discuss (or show with equations) how NO is formed in the human body and what effects is has.Explanation / Answer
2. Energy of photon of wavelength 546 nm (5.46 x 10^-7 m)
= hc/l
= 6.626 x 10^-34 x 3 x 10^8/5.46 x 10^-7
= 3.64 x 10^-19 J
energy of 1 mole of photon = 3.64 x 10^-19 x 6.023 x 10^23
= 2.19 x 10^5 J
color of light = yellow
8.Electronegativity is a term used in bonding, which is the ability of an atom to pull the shared pair of electrons towards itself in a bond. Say in water, Oxygen being more elecrtronegative pulls shared pair of electrons towards itself making Hydrogen slightly electropositive in nature. This charge separation gives a partial positive charge on hydrogen and a partial negative charge on oxygen making the bond polar and thus water is a polar molecule. On the other hand, carbon which is slightly more electronegative pulls electron towards itself, but the polarity generated by one C-H bond gets cancelled by other C-H bond on other side. So CH4 is a non-polar molecule. This effect does not exist in water wherein, the lone pair of electrons makes the geometry as bend so polarity of one O-H does not get cancelled by other O-H bond.
9. Ionic bond compounds : NaCl, CaCO3
Covalent bond compounds : CH4, C2H6
Ionic bonds are formed when electrons are completely transferred from one atom to another.
Covalent bonds are formed when two atoms share pair of electrons among them.
11. Reaction butane and oxygen
2C4H10 + 13O2 --> 8CO2 + 10H2O
moles butane = 100g/58 g/mol = 1.724 mol
grams CO2 formed = 1.724 x 8 x 44/2 = 303.45 g
grams of H2O produced = 1.724 x 10 x 18/2 = 155.16 g
12. Reaction of sodium with H2O
Is an oxidation of sodium metal from 0 to +1 oxidation state
Equation, 2Na + 2H2O ---> 2NaOH + H2 (g)
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