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Questions and Answers
What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? The value of $\lambda$ = ______
What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? The value of $\lambda$ = ______
$5.80 x 10^{-7}$ m
What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? The unknown (what you are solving for) is?
What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? The unknown (what you are solving for) is?
frequency
What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? The symbol for the unknown is?
What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? The symbol for the unknown is?
(\nu)
What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? What is the equation you will use to solve the problem?
What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? What is the equation you will use to solve the problem?
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What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? Any constant you will use, what is it?
What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? Any constant you will use, what is it?
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What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? What is the value of the constant?
What is the frequency of radiation if its wavelength is $5.80 x 10^{-7}$ m? What is the value of the constant?
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What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? The value of $\lambda$ = ______
What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? The value of $\lambda$ = ______
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What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? The unknown (what you are solving for) is?
What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? The unknown (what you are solving for) is?
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What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? The symbol for the unknown is?
What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? The symbol for the unknown is?
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What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? The equation you will use to solve problem is?
What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? The equation you will use to solve problem is?
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What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? Any constants you will use, what are they?
What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? Any constants you will use, what are they?
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What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? What are the values for the constants?
What is the energy of light if its wavelength is $4.25 x 10^{-7}$ m? What are the values for the constants?
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What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? The value of energy = ______
What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? The value of energy = ______
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What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? The symbol for energy =?
What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? The symbol for energy =?
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What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? The unknown (what you are solving for) is?
What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? The unknown (what you are solving for) is?
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What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? The symbol for the unknown is?
What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? The symbol for the unknown is?
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What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? The equation you will use to solve problem is?
What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? The equation you will use to solve problem is?
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What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? Any constant values you will use, what are they?
What is the frequency of light if its energy is $4.25 x 10^{-19}$ J? Any constant values you will use, what are they?
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If the energy of light is $6.15 x 10^{-19}$ J, what would be the wavelength of this light?
If the energy of light is $6.15 x 10^{-19}$ J, what would be the wavelength of this light?
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Draw an absorption energy level diagram for an electron at the ground state level of n = 2 and transitions to n = 5. Label the parts of the diagram (energy axis, ground state, excited state, light coming in, electron transition)
Draw an absorption energy level diagram for an electron at the ground state level of n = 2 and transitions to n = 5. Label the parts of the diagram (energy axis, ground state, excited state, light coming in, electron transition)
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Draw an emission energy level diagram for an electron at an excited state level of n = 4 and transitions to n = 1. Label the parts of the diagram (energy axis, ground state, excited state, light coming out, electron transition)
Draw an emission energy level diagram for an electron at an excited state level of n = 4 and transitions to n = 1. Label the parts of the diagram (energy axis, ground state, excited state, light coming out, electron transition)
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Draw a Bohr diagram for sulfur, S. Include electrons in diagram. # electrons are in sulfur?
Draw a Bohr diagram for sulfur, S. Include electrons in diagram. # electrons are in sulfur?
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Draw a Bohr diagram for sulfur, S. Include electrons in diagram. # of energy levels
Draw a Bohr diagram for sulfur, S. Include electrons in diagram. # of energy levels
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Draw a Bohr diagram for sulfur, S. Include electrons in diagram. # valence electrons?
Draw a Bohr diagram for sulfur, S. Include electrons in diagram. # valence electrons?
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Draw a Bohr diagram for sulfur, S. Include electrons in diagram. Energy level where valence electrons can be found?
Draw a Bohr diagram for sulfur, S. Include electrons in diagram. Energy level where valence electrons can be found?
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Draw the following orbitals. Make sure to label the axes: pz
Draw the following orbitals. Make sure to label the axes: pz
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If n = 3, what are the possible values of l?
If n = 3, what are the possible values of l?
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Draw an energy level diagram that include the orbitals, 1s, 2s, 2p, 3s, 3p, 3d, 4s, and 4p. Then fill the orbitals with electrons (arrows) corresponding to the element chromium. (Hint: start with the lowest energy)
Draw an energy level diagram that include the orbitals, 1s, 2s, 2p, 3s, 3p, 3d, 4s, and 4p. Then fill the orbitals with electrons (arrows) corresponding to the element chromium. (Hint: start with the lowest energy)
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Write the electron configuration and the orbital diagrams for Carbon, C
Write the electron configuration and the orbital diagrams for Carbon, C
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Write the electron configuration and the orbital diagrams for Oxygen, O
Write the electron configuration and the orbital diagrams for Oxygen, O
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Write the electron configuration and the orbital diagrams for Sodium, Na
Write the electron configuration and the orbital diagrams for Sodium, Na
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Write the electron configuration and the orbital diagrams for Phosphorus, P
Write the electron configuration and the orbital diagrams for Phosphorus, P
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Write the electron configuration and the orbital diagrams for Titanium
Write the electron configuration and the orbital diagrams for Titanium
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Write the electron configuration and the orbital diagrams for Arsenic, As
Write the electron configuration and the orbital diagrams for Arsenic, As
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Determine the number of valence electrons for Magnesium
Determine the number of valence electrons for Magnesium
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Determine the number of valence electrons for Chlorine
Determine the number of valence electrons for Chlorine
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Determine the number of valence electrons for Silicon
Determine the number of valence electrons for Silicon
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Circle the ions that are isoelectronic with argon, Ar.
Circle the ions that are isoelectronic with argon, Ar.
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For each pair, circle the element or ion that has a larger radius: Mg or Al
For each pair, circle the element or ion that has a larger radius: Mg or Al
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The decrease in the atomic radii of the elements in this table can best be explained by:
The decrease in the atomic radii of the elements in this table can best be explained by:
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Sulfur is in group 4B of the Periodic Table and normally holds 4 valence electrons before it reacts with other elements. Which of the following electron configurations matches sulfur?
Sulfur is in group 4B of the Periodic Table and normally holds 4 valence electrons before it reacts with other elements. Which of the following electron configurations matches sulfur?
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Calcium has an electron configuration of $1s^22s^22p^63s^23p^64s^2$. Based on this information, how many valence electrons does calcium have?
Calcium has an electron configuration of $1s^22s^22p^63s^23p^64s^2$. Based on this information, how many valence electrons does calcium have?
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Flashcards
Wavelength (λ)
Wavelength (λ)
The distance between successive peaks in a wave.
Frequency (ν)
Frequency (ν)
The number of waves that pass a point in a second.
Energy (E)
Energy (E)
The capacity to do work; in light, related to frequency and wavelength.
Planck's constant (h)
Planck's constant (h)
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c (Speed of light)
c (Speed of light)
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Energy-Wavelength Relationship
Energy-Wavelength Relationship
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Ionization Energy
Ionization Energy
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Atomic Radius
Atomic Radius
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Valence Electrons
Valence Electrons
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Isoelectronic
Isoelectronic
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Absorption Spectrum
Absorption Spectrum
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Emission Spectrum
Emission Spectrum
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Electron Configuration
Electron Configuration
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Nuclear Charge
Nuclear Charge
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Periodic Trend
Periodic Trend
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Ground State
Ground State
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Excited State
Excited State
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P, d Orbitals
P, d Orbitals
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Electron Transition
Electron Transition
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Chemical Bond
Chemical Bond
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Electronegativity
Electronegativity
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Chemical Radius Effect
Chemical Radius Effect
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Larger Radius Elements
Larger Radius Elements
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Valence Electron Count
Valence Electron Count
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Energy Level Diagrams
Energy Level Diagrams
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Step by Step Problem Solving
Step by Step Problem Solving
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Periodic Table Organization
Periodic Table Organization
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Chemical Properties of Nonmetals
Chemical Properties of Nonmetals
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Ionization Energy Trend
Ionization Energy Trend
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Group Trends
Group Trends
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Study Notes
Chemistry Unit 1 Recap
- Unit Conversions: 1 nm = 1.00 x 10⁻⁹ m
- Equations:
- E = hv
- c = 3.00 x 10⁸ m/s
- h = 6.626 x 10⁻³⁴ J⋅s
- E = hc/λ
- c = λν
Problem Solving Steps (General Example)
- Understand the Question: Identify the given information (variables) and what needs to be calculated (unknown variable)
- Identify Unknown Variable: Determine what you are solving for—frequency (ν), energy (E), or wavelength (λ).
- Choose the Correct Equation: Select the relevant equation from the provided equations (e.g. E =hv, E=hc/λ )
- Identify Constants: Determine the values of any constants needed (like c and h)
- Plug in Values and Solve: Substitute the known values into the equation and solve for the unknown variable.
- Show Steps: Clearly show all steps of your calculations.
Problem 1: Frequency of Radiation
- Given wavelength (λ) = 5.80 x 10⁻⁷ m
- Unknown: Frequency (ν)
- Equation: c = λν
- Constants: c = 3.00 x 10⁸ m/s
- Solve: Calculate ν by rearranging the equation: ν = c/λ; ν = (3.00 x 10⁸ m/s) / (5.80 x 10⁻⁷ m) = 5.17 x 10¹⁴ Hz
Problem 2: Energy of Light
- Given wavelength (λ) = 4.25 x 10⁻⁷ m
- Unknown: Energy (E)
- Equation: E = hc/λ
- Constants:
- h = 6.626 x 10⁻³⁴ J⋅s
- c = 3.00 x 10⁸ m/s
- Solve: Calculate E by plugging in known values and solving the equation. E = (6.626 x 10⁻³⁴ J⋅s)(3.00 x 10⁸ m/s) / (4.25 x 10⁻⁷ m) = 4.68 x10⁻¹⁹ J.
Problem 3: Frequency of Light from Energy
- Given energy (E) = 4.25 x 10⁻¹⁹ J
- Unknown: Frequency (ν)
- Equation: E = hv
- Constants: h= 6.626 x 10⁻³⁴ J⋅s
- Solve forν: ν = E/h = 4.25 x 10⁻¹⁹ J/ 6.626 x 10⁻³⁴ J⋅s = 6.42 x10¹⁴ Hz
Problem 4: Wavelength of Light from Energy
- Given energy (E) = 6.15 x 10⁻¹⁹ J
- Unknown: Wavelength (λ)
- Equation: E=hc/λ
- Constants: h, c
- Solve for λ : λ = hc/E = (6.626 x 10⁻³⁴ J⋅s *3.00 x 10⁸ m/s) / (6.15 x 10⁻¹⁹ J) = 3.22 x10⁻⁷ m
Additional Concepts
- Energy Level Diagrams: Diagrams illustrating energy levels of electrons in atoms. Transitions between energy levels correspond to absorption or emission of light.
- Bohr Diagrams: Diagrams showing the structure of atoms, including the nucleus & electron distribution in energy levels.
- Atomic Orbitals: Specific regions in space where electrons have a high probability of being found. (e.g. 1s, 2s, 2p, 3s, 3p, 3d, 4s, 4p).
- Electron Configurations and Orbital Diagrams: Representations of the arrangement of electrons in atoms' orbitals.
- Isoelectronic: Ions having the same electron configuration as a neutral noble gas (e.g. Ar).
- Atomic Radius: The size of an atom. Trends include increase down a group and decrease across a period.
- Ionization Energy: Energy required to remove an electron from an atom in the gaseous state. Trends in ionization increase across a period while decrease down a group.
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Description
Test your understanding of key concepts from Chemistry Unit 1. This quiz covers important unit conversions and equations needed to solve problems related to frequency, energy, and wavelength. Utilize the provided problem-solving steps to guide you through the calculations.
