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Chemistry Ch. 5
| Question | Answer |
|---|---|
| What couldn't Rutherford's Atomic Model explain? | The chemical properties of elements. |
| Explaining what leads to the chemical properties of elements required a model that better described the... | Behavior of electrons in atoms. |
| Who was Niels Bohr? | A young Danish physicist who developed his own atomic model. |
| How did Niels Bohr's model differ from Rutherford's? | He changed Rutherford's model to incorporate newer discoveries about how the energy of an atom changes when the atom absorbs or emits light. |
| What did Bohr propose in his model of the atom? | Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus. |
| Define energy levels. | The fixed energies an electron can have. |
| Electrons cannot _____ _______ energy levels. | Exist between. |
| To move from one energy level to another, an electron must... | Gain or lose just the right amount of energy. |
| Define a quantum. | A measurement of the amount of energy required to move an electron form one energy level to another energy level. |
| The higher energy levels are... | Closer together. |
| It takes less energy to... | Move up an energy level towards the top. |
| Define the Quantum Mechanical Model. | The modern description of the electrons in atoms. |
| What does the quantum mechanical model determine about the electrons in an atom? | The quantum mechanical model determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus of an atom. |
| Define an atomic orbital. | A mathematical expression that describes the probability of finding an electron at various locations around the nucleus. |
| The energy levels of electrons in the quantum mechanical model are labeled by... | Principal quantum numbers (n). |
| How do sublevels of principal energy levels differ? | Each energy sublevel corresponds to one or more orbitals of different shapes. The orbitals describe where an electron is likely to be found. |
| What shape are s orbitals? | Spherical. |
| What shape are p orbitals? | Dumbbell-shaped. |
| What shape are d orbitals? | Cloverleaf shapes. |
| What are the number of sublevels in the following principal energy levels? 1.) n=1. 2.) n=2. 3.) n=3. 4.) n=4. | 1.) 1. 2.) 2. 3.) 3. 4.) 4. |
| Define electron configurations. | The ways in which electrons are arranged in various orbitals around the nuclei of atoms. |
| What are the three rules for writing the electron configurations of elements? | The Aufbau Principle, the Pauli Exclusion Principle, and Hund's Rule. |
| What is the Aufbau Principle? | States that the electrons occupy the orbitals lowest energy level first. |
| What is the Paul Exclusion Principle? | States that an atomic orbital may describe at most two electrons. |
| Define spin. | A quantum mechanical property of electrons and may be thought of as a clockwise or counterclockwise. |
| What is Hund's Rule? | Every orbital must get an electron before one is completely filled. |
| Define amplitude. | The wave's height from zero to the crest. |
| Define wavelength. | The distance between the crests. -Represented by lambda (kinda looks like a backwards h). |
| Define frequency. | The number of wave cycles to pass a given point per unit of time. The units of frequency are usually cycles per second. -Represented by nu (almost identical to v). |
| The SI unit of cycles per second is called the... | Hertz. -A hertz can also be expressed as a reciprocal second (s^-1). |
| The product of frequency and wavelength equals... | A constant (c), the speed of light. |
| What is the equation for the speed of light? | C= Frequency x Wavelength. |
| The wavelength and frequency of light are... | Inversely proportional to each other. |
| As wavelength of light increases, the frequency... | Decreases. |
| What does electromagnetic radiation consist of? | -Radio Waves. -Microwaves. -Infrared Waves. -Visible Light. -Ultraviolet Waves. -X-Rays. -Gamma Rays. |
| All electromagnetic waves travel in a vacuum speed of... | 2.998 x 10^8 m/s. |
| Define spectrum. | When sunlight passes through a prism, the different wavelengths separate into a spectrum of colors. |
| What causes atomic emission spectra? | When atoms absorb energy, their electrons move to higher energy levels. These electrons lose energy by emitting light when they return to lower energy levels. |
| The energy absorbed from an electron for it to move from its current energy level to a higher energy level is identical to... | The energy of light emitted by the electron as it drops back to its original energy level. |
| All wavelengths of visible light are _______ ________. | Blurred Together. |
| The wavelengths of spectral lines are characteristic of the element, and they make up the _________ _________ _________ of the element. | Atomic Emission Spectrum. |
| Each spectral line in an atomic emission spectrum of an element corresponds with... | Exactly one wavelength of light emitted by the electrons of that element. |
| True or false: No two elements have the same atomic emission spectrum. | True. |
| Who was Max Planck? | A German physicist who found that he could explain the color changes if he assumed that the energy of a body changes only in discrete units, or quanta. |
| What did Planck show? | Planck showed mathematically that the amount of radiant energy (E) of a single quantum absorbed or emitted by a body is proportional to the frequency of radiation (v). |
| What is the equation for radiant energy? | E= C x V. C equals Constant and has a value of 6.626 x 20^-34 Joules time seconds. V equals Frequency of Radiation. |
| What happens during the photoelectric effect? | Electrons are ejected when light shines on a metal. |
| What did Einstein propose to explain the photoelectric effect? | Einstein proposed that light could be described as quanta of energy that behave as if they were particles. |
| What are photons? | Light quanta. |
| If no electrons are ejected, what does this tell us? | The frequency of the light is below the threshold frequency. |
| If the light is at or above the threshold frequency, then what happens? | Electrons are ejected. |
| If the frequency is increased, what will happen when the electrons are ejected? | The ejected electrons will travel faster. |
| What was Democritus's atomic theory and atomic model? | None. But, he did coin the term "atomos", which means indivisible or atoms. |
| What was Dalton's atomic theory and atomic model? | Kinetic Theory and the sphere. |
| What does the Kinetic Theory state? | 1.) Everything is made of atoms. Can't be destroyed, 2.) All atoms of an element are identical. 3.) The atoms of a different element vary in size and mass. 4.) Compounds are made with different whole # combos. 5.) Chemical react= rearranged atoms. |
| What was Thomson's atomic theory and atomic model? | Used the cathode ray to find the first subatomic particle. It had a negative charge and was called the electron. Plum pudding model. |
| What was Millikan's atomic theory and atomic model? | Electrons have a mass of 9.109 x 10^(-31) kg. Also used the plum pudding model. |
| What was Rutherford's atomic theory and atomic model? | Atoms are mostly empty space, dense nucleus, found the 2nd subatomic particle, the proton, which had a mass of 1.67 x 10^(-27). His model was the plum pudding with positive, dense center. |
| What was Chadwick's atomic theory and atomic model? | A neutron had a mass of 1.65 x 10^(-27) kg. His model was the plum pudding with positive, dense center. |
| What was Bohr's atomic theory and atomic model? | Quanticized. Energy levels 2n^2. Energy level on the periodic table. His model was the "solar system". |
| What was DeBroglie's atomic theory and atomic model? | Quantum theory where the electrons exhibit wave behavior. "Flower" model. |
| What was Heisenberg's atomic theory and atomic model? | Cannot know both the location and velocity of an electron at the same time. "Flower" model. |
| What was Schrodinger's atomic theory and atomic model? | Packets of energy and particles with mass. "Flower" model. |
| Define atomic orbital. | Probaic region to find an electron. |
| What is the principle quantum? What's the symbol? | Coinsides with the periods on the periodic table. Determins size of atomic orbital. (2n^2). Fill the lowest energy level first, then take a jump from ground state, electrons need energy to move up, and you remove energy to go down. -n. |
| What is ground state? | The lowest energy level. |
| What is the angular momentum? What's the symbol? | Subshells, letter designations, and shapes. -L. |
| What are the shapes for the s, p, d, and f orbitals? | -S-Orbital: Sphere. -P-Orbital: Eight or infinity sign. -D-Orbital: Eight with backup. -F-Orbital: Flower in cube. |
| What is the magnetic quantum What's the symbol? | Holds two electrons. Orientation in space. -ML. |
| The magnetic quantum has 3 categories. What are they? | -X-Axis : Horizontal. -Y-Axis: Vertical. -Z-Axis: Toward or Away. |
| What is the Spin Magnetic Quantum? What is the symbol? | Specifies the electrons in orbitals. Has a special set of rules. -Ms. |
| What is Aufbau's Principle? | You must fill the lowest energy level first. |
| What is Pauli Exclusion Principle? | No two electrons in the same atom can have the same set of 4 quantum numbers, or, an orbital can hold at most 2 electrons. |
| What is Hund's Rule? | Electrons occupy orbitals of equal energy one-at-a-time with the same spin until each orbital has at least one electron. -Can't give my best friend 2 cookies until everyone has had one. |
| Define Quantum. | The amount of energy need for an electron to move up or down an energy level. |
| What are the three electron notations? | 1.) Orbital Notation. 2.) Electron Configuration Notation. 3.) Noble Gas Notation. |
| What is Orbital Notation? | Uses half arrows to represent electrons in subshells and lines to represent the orbital. |
| What is Electron Configuration Notation? | Uses coefficients for energy levels, the letter designations, orbital, and superscript for the number of electrons present. |
| What is Noble Gas Notation? | Uses the noble gas element preceding the current element. Write that noble gas in brackets and finish the electron configuration post noble gas. |
| What is the Octet Rule? | Want 8 electrons in valence energy shell. |
| What is the speed of light? | 2.99 x 10^8 m/s. |
| What is the equation for speed of light? | C=Wavelength (m) x Frequency (Hz). |
| __________ _________ _________ grew out of the study of light. | Quantum Mechanical Model. |
| What is a wave? | A wave cycle starts at zero on the y-axis, moves up to its highest point. |
| What is amplitude? | The highest or lowest point. |
| What is frequency? | Wave cycle between a certain unit of time. |
| What is a crest? | The highest point of a wave. |
| What is a trough? | The lowest point of a wave. |
| A longer wavelength means a _______ frequency. | Lower. |
| A shorter wavelength means a _______ frequency. | Higher. |
| What is the order of the Electromagnetic Spectrum? (Lowest to Highest). | Radio Waves, Microwave, Infrared, Ultra-Violet, X-Rays, Gamma Rays. |
| What is the blue shift? | Compress the wavelength. |
| What is the red shift? | Stretch the wavelength. |
| What is the Atomic Emission Spectra? | When atoms absorb energy, their electrons move to higher energy levels. |
| The energy required for an electron to move up is identical to the... | Amount emitted to move down. |
| True or false: All AES are the same. | False, AES are unique and act as fingerprints to identify elements. |
| What are the three points Einstein used to explain the Photoelectric Effect? | 1.) Classical Physics. 2.) Quantization of Energy. 3.) The Photoelectric Effect. |
| What is the classical physics point? | Atomic emission spectrum should be continuous does not explain spectra of atoms, which consist of lines. |
| What is the quantization of energy point? | Described mathematically that the amount of radiant energy (E) of a single quantum absorbed or emitted by a body is proportional to the frequency of radiation (v). |
| Who created the quantization of energy point? | Maxwell Planck. |
| What is the photoelectric effect point? | Light could be described as quanta of energy that behave as if they were particles. |
| What equations is used for energy/photons? | E=Plancks Constant(Jxs) x Frequency(per second). |
| What's Planck's Constant? | 6.626 x 10^(-34) Jxs |
| In the photoelectric theory, the smaller change means... While large change means... | Lower frequency. -Higher frequency. |
| Einstein proposed there was a ________. | Threshold. |
| How are the frequencies of light emitted by an atom related to changes of electron energies? |
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OliviaRoark
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