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42 Cards in this Set
- Front
- Back
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identify characteristics of a wave and explain relationships between some of these characteristics
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k
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organize parts of the visible and electromagnetic spectra according to wavelength, frequency or energy
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radio waves
micro waves infra red red orange yellow green blue indigo violet ultra violet x ray gamma ray |
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explain the photoelectric effect and how it can be used to produce electricity
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higher frequencies of light are able to knock electrons off a metal surface
-light must act as particles if it is able to "knock" electrons free -the movement of electrons creates light -helps explain the quantum theory |
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photon
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a particle/ quantum of light energy
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describe how a line spectrum forms
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when an electron is in an excited state and has just enough energy, it can jump to a lower energy level and when it does this it releases the excess energy creating a line spectra in which we see as light
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explain quantum theory, and why we do not notice these quanta in everyday situations
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energy travels in small pieces or bundles and those bundles are called a quantum; they are so small we cannot notice them
-each quantum must be full - no halves -there is a fundamental restriction on the amounts of energy that an object emits or absorbs; meaning that there cannot b ea pause between hits or if it was going to go back and stop halfway |
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describe the wave mechanical model of the atom
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-the act of measuring the location of an electron make it move making it impossible to describe the exact location of electrons; mathematical models are able to describe wave properties of electrons
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list and explain all the rules for the distribution of electrons in an atom
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1. aufbau principle
2. hund's rule 3. pauli exclusion rule 4. diagonal rule |
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list each sublevel, how many electrons it can hold, and its shape
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s sublevels contain one orbital; spherical
p sublevels contain 3 orbitals; peanut d sublevels contain 5 orbitals; four leaf clover f sublevels contain 7 orbitals; complex |
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know how to do electron configurations
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l
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recognize patterns of electron configurations on the periodic table
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l
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write noble gas configurations
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o
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sub level
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all of the orbitals and their electrons of that letter such as P
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aufbau principle
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-electrons are added to the lowest energy sublevel, one at a time, until that sublevel is full
-this process continues until all electrons in the atom have been accounted for |
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orbital diagram
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shows the sublevels and the electrons spins
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quantum
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small pieces or bundles
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orbital
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the area within an energy level where the electron is most likely found
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electron spin
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must go in opposite positions to be in the same orbital
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pauli exclusion principle
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an orbital can hold a maximum of 2 electrons
-in order to do this, the electrons must have opposite spins |
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energy level
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all of the same numbers including their letters such as 2s and 2p which would be an energy level
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electron configuration
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distribution of electrons among the orbitals in an atom; where the electrons are most likely found - where they are organized into energy levels, sublevels, and other orbitals according to a set of rules
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hund's rule
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electrons occupy equal energy orbitals so a maximumnumber of unpaired electrons exist
-paired electrons = 2 in teh same orbital -unpaired = 1 electron in an orbital |
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wavelength
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the distance between successive crests of the wave; the wave travels as it completes one full cycle of upward and downward motion
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frequency
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tells how fast the wave oscillate up and down; the number of waves that pass a point in one second; frequency and wavelength are inversely related
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amplitude
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the height of the wave measured from the origin to its crest or peak; affects brightness and intensity of light
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wave period
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how long it takes to pass a certain point
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crest
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peak of each wave
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trough
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bottom of each wave
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speed of light
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3.00 x 10(8 exponent) m/s
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electromagnetic spectrum
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describes all wavelengths of light
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line spectrum
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a spectrum that contains only certain colors or wavelengths; ex: fireworks emitting specific colors
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continuous spectrum
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interval of real numbers;
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wave particle duality
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a postulate that all particles exhibit both wave and particle properties
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photoelectric effect
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higher frequencies of light are able to knock electrons off a metal surface; light must act as particles if it is able to "knock" electrons free; helps explain the quantum theory
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wave mechanical model
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the act of measuring the location of an electron makes it move making it impossible to describe the exact location of electrons - mathematical models are able to describe wave properties of electrons
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valence electrons
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electrons in the outermost energy level
-usually consists of a maximum of 8 |
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ionic size
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radius of an atoms ion
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ionization energy
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the energy needed to remove the outermost electron from the atom; high energy - they want to give one away or they want one more
low - they want to give their away b/c they have too many and want a full shell vertical - high energy at the top, low at the bottom horizontal - high at the right and low and the left |
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highest ionzation energy and lowest
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helium is highest
francium is lowest |
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what elements want to gain and what want to lose
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metals - going to lose
non metals - want to gain |
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when there is 4 electrons......
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non metals - gain
metals - lose |
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diagonal rule
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-larger energy levels overlap
-some sublevels in higher energy levels fill before sublevels in lower energy levels -use a diagonal rule or periodic table to predict energy level overlap |
