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This document contains 6 questions about general chemistry concepts including: 1) The maximum number of electrons that can occupy atomic subshells and quantum numbers 2) Writing condensed electron configurations and determining unpaired electrons for various atoms 3) Calculating frequency and wavelength from each other 4) Labeling statements about electromagnetic radiation as true or false 5) Calculating and comparing photon energies at different wavelengths 6) Drawing the electromagnetic spectrum.
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This document contains review questions covering topics in waves, emission and the Bohr model, electrons, and photon properties. It asks about wavelength, Planck's constant, the speed of light, electron configurations for various elements, filling electron orbitals according to Aufbau principle, converting between units of length and frequency, and using formulas relating energy, Planck's constant, frequency, and wavelength of electromagnetic waves including photons.
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Unit 1 lesson 12ppt
When a neutral atom loses or gains electrons, it is no longer neutral. It becomes an ion that has a positive or negative charge depending on whether electrons were lost or gained:
- Losing electrons leaves the atom with more protons than electrons, giving it a positive charge. It is now a positive ion.
- Gaining electrons leaves the atom with more electrons than protons, giving it a negative charge. It is now a negative ion.
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#26 Key
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#32
The document contains 8 questions about general chemistry concepts including:
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The document discusses concepts in general chemistry including effective nuclear charge, electron configuration, atomic and ionic sizes, and ionization energies. It defines effective nuclear charge as the charge felt by an electron from the nucleus and how it decreases across a period as nuclear charge is shared by more electrons. It asks about the electron configuration, valence electrons, and energy level of magnesium as well as how its effective nuclear charge differs from carbon. Finally, it asks about writing equations for specific ionization energies of tin and titanium.
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The document discusses key concepts in general chemistry including:
1) Effective nuclear charge increases left to right and down a period, lowering electron energy due to stronger electrostatic attraction but increasing it due to greater electron-electron repulsion.
2) Magnesium has an electron configuration of [Ne]3s2, with 2 valence electrons and an effective nuclear charge of +2.
3) Atomic radius generally decreases left to right and increases down a period, while ionic radius follows the opposite trends due to shielding effects.
#30 Key
The document provides information about trends in the periodic table including:
1) Ion size increases down a column due to increasing nuclear charge.
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3) Ionization energy decreases down a group and increases across a period as nuclear charge increases.
4) Reactivity of alkali metals increases down a group as electrons are more readily removed further from the nucleus.
#26
The document contains questions about fundamental concepts in general chemistry including:
1) The formula for the energy of a photon.
2) The ground and excited states of a photon.
3) Definitions of key terms like wave function, probability density, orbitals, electron shells, subshells, degeneracy, Pauli exclusion principle, electron configuration, and Hund's rule.
4) Tables to fill in about quantum numbers and maximum possible electrons in different orbitals.
5) Questions about the values of quantum numbers n, l, and ml for different orbitals.
6) Determining electron configurations using both longhand and shorthand notation for various elements.
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1. An object can possess energy in two ways: potential energy due to position or configuration, and kinetic energy due to motion. Potential energy is stored energy due to factors like height or chemical composition, while kinetic energy is energy due to an object's motion.
2. A kilowatt-hour is equal to 3,600,000 joules. An adult radiates heat at about 100 watts, so in 24 hours would radiate 24,000 kcal of energy to the surroundings.
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This document contains a chemistry practice test with multiple choice and free response questions about periodic trends, ion formation, Lewis structures, the octet rule, and electronegativity. Some key points covered are:
1. Metal character increases down a group and decreases across a period on the periodic table. Metals have low ionization energies.
2. Group 1A metals form 1+ ions and group 2A metals form 2+ ions. Most metal oxides are basic while most nonmetal oxides are acidic.
3. The octet rule states that main group elements gain, lose, or share electrons to achieve an octet of 8 electrons in their valence shell. Not all molecules obey this rule
#27 Key
1. The maximum number of electrons that can occupy each subshell is: 3p = 6, 5d = 10, 2s = 2, 4f = 14.
2. The maximum number of electrons for the given quantum numbers are: a) n = 2, ms = -1/2 is 3 electrons, b) n = 5, l = 3 is 14 electrons, c) n = 4, l = 3, ml = -3 is 2 electrons, d) n = 4, l = 1, ml = 1 is 2 electrons.
3. The electromagnetic spectrum ranges from high energy gamma rays and x-rays to lower energy radio waves.
#23
The document is a study guide for a general chemistry exam that includes 8 questions covering topics like:
1) Calculating enthalpy changes for chemical reactions using given enthalpy of formation values
2) Calculating standard enthalpy change values (ΔH°) for chemical reactions using reference tables
3) Calculating standard enthalpy of formation for diborane gas using thermochemical data
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#32 Key
The document summarizes key concepts in general chemistry including:
1) Tetrahedral molecules like methane and perchlorate ion have bond angles of 109.5 degrees. Trigonal pyramidal ammonia requires specifying two parameters - the H-N-H bond angle and N-H bond distance.
2) The number of electron domains is determined by counting bonds and lone pairs. Bonding domains contain bonding electrons while nonbonding domains contain lone pairs.
3) Molecules with 3, 4, 5, or 6 electron domains exhibit trigonal planar, tetrahedral, trigonal bipyramidal, or octahedral electron domain geometries respectively.
4) Electron domain angles of
#31 Key
1) Metal character increases down a group and decreases across a period on the periodic table. Metals have low ionization energies and form cations by losing electrons.
2) Most metal oxides are basic, while most nonmetal oxides are acidic. When nonmetal oxides react with water, acids are formed.
3) The octet rule states that atoms bond to achieve a full outer shell of 8 electrons. Atoms gain, lose or share electrons to achieve an octet configuration.
#23 Key
1. Calculate the enthalpy change for the reaction P4O6 (s) + 2 O2 (g) → P4O10 (s) using given enthalpy values for related reactions.
2. Calculate the standard enthalpy of reaction (ΔH°) for several reactions using standard enthalpies of formation from appendix C.
3. Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using thermochemical cycles and given reaction enthalpies.
4. Explain the meaning of "fuel value" and determine whether 5 g of fat or 9 g of carbohydrates provides more energy as food using their fuel
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The document provides instructions for building dot structures to represent the molecules ammonia (NH3) and carbon dioxide (CO2):
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2) Add up the valence electrons of each atom. NH3 has a total of 8 electrons from nitrogen and hydrogen. CO2 has a total of 16 electrons from carbon and oxygen.
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This document is a learning package that supplements classroom learning for students working independently. It contains various activities and exercises about concepts related to electron configuration and orbitals that are intended to deepen understanding. The package instructs students to complete the activities independently and honestly, writing their answers on paper and comparing to an answer key after attempting each task.
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An atom is composed of a small, positively charged nucleus surrounded by negatively charged electrons. The nucleus contains protons and neutrons, with protons determining the element and having a positive charge. Electrons orbit the nucleus and provide neutrality to the atom through their negative charge balancing out the positive charge of the protons. Different elements are distinguished by their atomic number, which is the number of protons in the nucleus.
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The document contains 8 questions about general chemistry concepts including:
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2) Determining the number of electron domains and the difference between bonding and nonbonding domains.
3) The characteristic electron-domain geometry of 3, 4, 5, and 6 electron domains around a central atom.
4) The number of electron domains implied by given bond angles.
5) Predicting if molecules are polar or nonpolar based on their structure.
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The document contains questions about trends in the periodic table including ion size, isoelectronic series, electron configuration of ions, ionization energy, electron affinity, reactivity of alkali metals, balancing equations for alkali metal oxide reactions, and properties of noble gases. It asks about trends in properties including ionic radius, ionization energy, metallic character, and molecular structure as one moves through the periodic table.
#29
The document discusses concepts in general chemistry including effective nuclear charge, electron configuration, atomic and ionic sizes, and ionization energies. It defines effective nuclear charge as the charge felt by an electron from the nucleus and how it decreases across a period as nuclear charge is shared by more electrons. It asks about the electron configuration, valence electrons, and energy level of magnesium as well as how its effective nuclear charge differs from carbon. Finally, it asks about writing equations for specific ionization energies of tin and titanium.
#29 Key
The document discusses key concepts in general chemistry including:
1) Effective nuclear charge increases left to right and down a period, lowering electron energy due to stronger electrostatic attraction but increasing it due to greater electron-electron repulsion.
2) Magnesium has an electron configuration of [Ne]3s2, with 2 valence electrons and an effective nuclear charge of +2.
3) Atomic radius generally decreases left to right and increases down a period, while ionic radius follows the opposite trends due to shielding effects.
#30 Key
The document provides information about trends in the periodic table including:
1) Ion size increases down a column due to increasing nuclear charge.
2) Elements with the same number of electrons form isoelectronic series.
3) Ionization energy decreases down a group and increases across a period as nuclear charge increases.
4) Reactivity of alkali metals increases down a group as electrons are more readily removed further from the nucleus.
#26
The document contains questions about fundamental concepts in general chemistry including:
1) The formula for the energy of a photon.
2) The ground and excited states of a photon.
3) Definitions of key terms like wave function, probability density, orbitals, electron shells, subshells, degeneracy, Pauli exclusion principle, electron configuration, and Hund's rule.
4) Tables to fill in about quantum numbers and maximum possible electrons in different orbitals.
5) Questions about the values of quantum numbers n, l, and ml for different orbitals.
6) Determining electron configurations using both longhand and shorthand notation for various elements.
#22
1. An object can possess energy in two ways: potential energy due to position or configuration, and kinetic energy due to motion. Potential energy is stored energy due to factors like height or chemical composition, while kinetic energy is energy due to an object's motion.
2. A kilowatt-hour is equal to 3,600,000 joules. An adult radiates heat at about 100 watts, so in 24 hours would radiate 24,000 kcal of energy to the surroundings.
3. For the chemical reaction of silver ions and chloride ions forming silver chloride: a) the heat of reaction for 0.200 mol of AgCl forming is -13.12 kJ; b) the
#31
This document contains a chemistry practice test with multiple choice and free response questions about periodic trends, ion formation, Lewis structures, the octet rule, and electronegativity. Some key points covered are:
1. Metal character increases down a group and decreases across a period on the periodic table. Metals have low ionization energies.
2. Group 1A metals form 1+ ions and group 2A metals form 2+ ions. Most metal oxides are basic while most nonmetal oxides are acidic.
3. The octet rule states that main group elements gain, lose, or share electrons to achieve an octet of 8 electrons in their valence shell. Not all molecules obey this rule
#27 Key
1. The maximum number of electrons that can occupy each subshell is: 3p = 6, 5d = 10, 2s = 2, 4f = 14.
2. The maximum number of electrons for the given quantum numbers are: a) n = 2, ms = -1/2 is 3 electrons, b) n = 5, l = 3 is 14 electrons, c) n = 4, l = 3, ml = -3 is 2 electrons, d) n = 4, l = 1, ml = 1 is 2 electrons.
3. The electromagnetic spectrum ranges from high energy gamma rays and x-rays to lower energy radio waves.
#23
The document is a study guide for a general chemistry exam that includes 8 questions covering topics like:
1) Calculating enthalpy changes for chemical reactions using given enthalpy of formation values
2) Calculating standard enthalpy change values (ΔH°) for chemical reactions using reference tables
3) Calculating standard enthalpy of formation for diborane gas using thermochemical data
4) Defining fuel value and comparing the energy provided by fat and carbohydrates
5) Calculating the caloric content of alcohol in wine using given ethanol content and heat of combustion values
6) Explaining why fats are suitable for energy storage and calculating the percentage of calories from fat in a
#32 Key
The document summarizes key concepts in general chemistry including:
1) Tetrahedral molecules like methane and perchlorate ion have bond angles of 109.5 degrees. Trigonal pyramidal ammonia requires specifying two parameters - the H-N-H bond angle and N-H bond distance.
2) The number of electron domains is determined by counting bonds and lone pairs. Bonding domains contain bonding electrons while nonbonding domains contain lone pairs.
3) Molecules with 3, 4, 5, or 6 electron domains exhibit trigonal planar, tetrahedral, trigonal bipyramidal, or octahedral electron domain geometries respectively.
4) Electron domain angles of
#31 Key
1) Metal character increases down a group and decreases across a period on the periodic table. Metals have low ionization energies and form cations by losing electrons.
2) Most metal oxides are basic, while most nonmetal oxides are acidic. When nonmetal oxides react with water, acids are formed.
3) The octet rule states that atoms bond to achieve a full outer shell of 8 electrons. Atoms gain, lose or share electrons to achieve an octet configuration.
#23 Key
1. Calculate the enthalpy change for the reaction P4O6 (s) + 2 O2 (g) → P4O10 (s) using given enthalpy values for related reactions.
2. Calculate the standard enthalpy of reaction (ΔH°) for several reactions using standard enthalpies of formation from appendix C.
3. Calculate the standard enthalpy of formation of gaseous diborane (B2H6) using thermochemical cycles and given reaction enthalpies.
4. Explain the meaning of "fuel value" and determine whether 5 g of fat or 9 g of carbohydrates provides more energy as food using their fuel
#22 Key
1. An object can possess energy through kinetic energy from its motion or potential energy from its position. Kinetic energy depends on mass and velocity while potential energy depends on position.
2. A kilowatt-hour equals 3.6 million joules. An adult radiates heat at the same rate as a 100-watt bulb, so in 24 hours they radiate about 2.1 kilocalories of heat energy.
3. Chemical reactions that release heat are exothermic, while those that absorb heat are endothermic. Heat change equals internal energy change during constant pressure processes.
#21 Key
The document defines key terms related to thermodynamics and calorimetry, including enthalpy, enthalpy of reaction, calorimetry, heat capacity, bomb calorimeter, Hess's law, enthalpy of formation, and standard enthalpy of reaction. It then provides examples of using these concepts to calculate enthalpy changes, heat transferred, and moles or mass of substances involved in various chemical reactions.
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