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71 Cards in this Set
- Front
- Back
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Isotopes have...
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same # of protons, but different # of neutrons
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Relationships between elements in the same family (column)
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They take on the same charge and bond in the same ratio with other elements
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What is an atomic mass unit
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1 proton or 1 neutron, used to measure average atomic mass
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What are the four characteristics of light?
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Speed, Wavelength, Amplitude, Frequency
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Define the four charcteristics
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Speed - how fast the light travels
Wavelength- distance from a wave's crest to crest Frequency - how often the peak of the wave hits you per second Amplitude - how bright the light is, height of the wave |
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Visible light that has the highest frequency is...
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Violet
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lowest frequency?
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Red
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Visible light with the longest wavelength is...
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Red
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Visible light with the shortest wavelength is...
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Violet
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Frequency is measured in...
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hertz, cycles/second, sec^-1, /second
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Wavelength is measured in, typically...
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meters or nanometers
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Fundamentally, a quanta is a piece or unit of...
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energy
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As frequency increases, the energy of light
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increases
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As wavelength increases, the frequency of light
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decreases
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As the frequency of light increases, the wavelength
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decreases
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E =
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hv = hc/wavelength
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c=
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v * wavelength
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What is h
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Planck's constant (6.626 * 10^-34 Js)
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What is c
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Speed of light (3.0 * 10^8 m/sec)
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Aufbau Principal
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Lower energy levels must be filled before higher ones
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Hund's Rule
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Each orbital of an equal energy level must contain one electron before doubling up
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Pauli Exclusion Principle
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Electrons must have opposite spins, each suborbital may only have a maximum of 2 electrons
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What properties separate metals from non-metals
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Luster, Conductivity of electricity, Conductivity of heat, Malleability, Ductility, Solid at room temperature (excluding Mercury)
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Malleability is the ability of a substance to be...
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hammered into a sheet
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Ductility is the ability of a substance to be
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formed into a wire
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Semi-metals are also called...
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Metalloids
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Atomic radius
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the distance from the center of the atom to the outside edge of an electron cloud
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Ionization Energy
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the energy required to remove an electron from an atom in its gaseous state
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Electronegativity
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the ability of an atom to attract electrons when the atom is in a compound
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Ionization energy increases on the periodic table as you go...
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left to right and bottom to top
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Atomic radius decreases on the periodic table as you go...
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left to right and bottom to top
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Electronegativity (ignoring noble gasses) decreases as you go...
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top to bottom and right to left
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Elements with the highest ionization energy
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noble gasses
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Elements with lowest ionization energy
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Alkali metals
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Mendeleev arranged the elements on the periodic table by...
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atomic mass
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Elements on the current periodic table are organized by
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atomic #
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Atomic Number =
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Number of protons in an atom
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Mass Number =
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# of protons + # of neutrons
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How does atomic mass differ from mass number?
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Atomic mass is the average mass of an element, while the mass number is just the mass of a single isotope of the element
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What are the four energy sublevels electrons can be in?
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s,p,d, or f sublevels
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Why are the spectras of three different elements different?
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This is because the electrons in each element can only get excited enought to get to certain energy levels and give off a certain wavelength of light, no more, no less
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Why is there not a continuous series of colors?
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Because, certain electrons can only give of certain wavelengths of light
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This means that electrons are...
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quantized - they can only have specific energies, nothing in between
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Visible light was a wavelength of
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between 400 and 750 nanometers
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Light acts as both a ......
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wave and a particle
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Electronegativity does not apply to...
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Noble gasses
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Why are alkali metals so highly reactive?
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This is because they hold onto their electrons the weakest (their ionization energy is low)
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Electronegativity applies ONLY to...
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things in bonds
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The Quantum mechanical Model is based on mathematical solutions from...
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The Schrodinger Equation
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Where in the atom do you find protons, neutrons, and electrons?
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Protons and neutrons are in the nucleus, while electrons are in an electron cloud around the nucleus
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How do you find average atomic mass?
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% abundance (as a decimal) * mass + % abundance * mass + % abundance * mass ....
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A group/family is in a...
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column
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A period is in a...
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row
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Periodic Law
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States that the periodic table is organized by atomic #
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Describe what happens when you heat/run electricity through an element in the gaseous state...
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Electrons absorb energy and jump to a higher energy level. This is their excited state. However, the electrons do not want to stay on the higher energy level, so they fall back down (ground state) and release energy (photon)
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What is a line spectrum?
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Set of colored lines formed when the light released by an energized element is passed through a prism
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photon
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particle of light
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What did Bohr study?
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The line spectrum of hydrogen gas
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ground state
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the lowest energy level an electron can be on
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excited state
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any energy level higher than the ground state
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What happens when an electron goes from the ground state to the excited state? The excited state to ground state?
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When an electron goes from the ground state to the excited state, it absorbs energy and it releases the energy as a photon when it goes from the excited state to the ground state
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What is the modern model of the atom called?
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The Quantum Mechanical Model
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What is an orbital?
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An area with a high probability of finding an electron
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What is an electron cloud?
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An area that surrounds the nucleus, in which there is a high probability of finding electrons
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What is the maximum number of electrons each energy level can hold?
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2n^2
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Which sublevels are on each energy level?
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n=1 has s, n=2 has s and p, n=3 has s,p,and d, n=4 has s,p,d,and f
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How many orbitals are in each sublevel?
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s=1, p=3, d=5, f=7
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Why are alkali metals so highly reactive?
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Because their electrons are very loosely bound, they have low ionization energies
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Lightbulbs give of so much light because...
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several electrons are getting excited and falling back to their ground states
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Electromagnetic Radiation
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Invisible light with longer wavelengths than visible light
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In the chromatography lab, why did some dyes move further up the page than others?
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This was because some dyes were more attracted to the alcohol mixture than others. So, they, therefore, went further up the page with the dye
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