| A | B |
|---|
| A form of energy that exhibits wavelike behavior as it travels through spacew like visible light, microwave, X-rays, TV and radio waves | electromagnetic radiation |
| the shortest distance between equivalent points on a continuous wave measured from crest to crest or trough to trough | wavelength |
| the number of waves that pass a given point per second | frequency |
| Equals one wave per second | one hertz |
| The waves height from the origin to the crest or from the origin to the trough | amplitude |
| the speed of all electromagnetic waves including visible light | 3.00 X 10 to the eigth m/s in a vacuum |
| What is the symbol for speed of light? | C |
| Product of its wavelength and its frequency | speed of light |
| Light that has a longer wavelength has... | a lower frequency |
| Light that has a shorter wavelength has a ....... | higher frequency |
| An example of white light that contains a continuous range of wavelengths and frequencies | sunlight |
| What happens when sunlight passes through a prism? | It is separated into a continuous spectrum of colors which are the colors of the visible spectrum |
| What is formed when tiny drops of water in the air disperse the white light from the sun into its component colors producing a continuous spectrum that arches across the sky? | a rainbow |
| All forms of electromagnetic radiation with different frequencies and wavelengths | electromagnetic spectrum |
| What results from shorter wavelengths bending more than longer wavelengths as they pass through the prism? | results in the sequence of colors red, orange, yellow, blue, indigo, and violet |
| How can you remember the sequence of colors? | Roy G. Biv |
| What happens to energy as the frequency increases? | Energy increases |
| How can you calculate the wavelength or frequency of any wave? | use the formula light speed equals wavelength times frequency. Frequency is v. |
| The minimum amount of energy that can be gained or lost by an atom? | quantum |
| He demonstrated mathematically that the energy of a quantum is related to the frequency of the emitted radiation by the equation energy=frequency times his constant. | Planck |
| According to his theory, for a given frequency, matter can emit or absorb energy only in whole number multiples of hv; that is 1 hv, 2 hv, 3 hv, and so on | Planck |
| Electrons, called photoelectrons, are emitted from a metal's surface when a light of a certain frequency shines on the surface | photoelectric effect |
| They power calculators by converting the energy of incident light into electrical energy | photoelectric cells |
| He proposed that electromagnetic radiation has both wavelike and particlelike natures. He calculated that a photon's energy depends on its frequency. | Einstein |
| a particle of electromagnetic radiation with no mass that carries a quantum of energy | photon |
| the set of frequencies of the electromagnetic waves emitted by atoms of the element | atomic emission spectrum |
| How is light produced in the glowing tubes of neon signs? | The light of a neon sign is produced by passing electricity through a tube filled with neon gas. Neon atoms in the tube absorb energy and become excited. The unstable atoms release energy by emitting light. |
| What is characteristic of the element being examined and can be used to identify that element? | the atomic emission spectrum |
| The fact that only certain specific frequencies of light are emitted means that .... | only certain specific frequencies of light are emitted |
| He proposed that the hydrogen atom has only certain allowable energy states | Bohr |
| What is the lowest allowable energy state of an atom called? | ground state |
| What state is an atom in when it gains energy? | excited state |
| How did Bohr suggest that the single electron in a hydrogen atom move around the nucleus? | only moves in certain circular orbits |
| The smaller the electron's orbit, the lower the | energy state or energy level |
| The larger the electron's orbit, the higher the | energy state or energy level |
| What does an atom emit corresponding to the difference between the energy levels associated with the two orbits? | a photon |
| Derived an equation for wavelength of a particle of mass (m) moving at velocity (V) and predicted that electrons and all moving particles do indeed have wave characteristics. | the de Broglie equation |
| States that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time | the Heisenburg uncertainty |
| What is the atomic model in which electrons are treated as waves? | quantum mechanical model of the atom or the wave mechanical model of the atom |
| A three-dimensional region around the nucleus that describes the electron's probable location? | atomic orbital |
| What does the Bohr atomic model assign to electron orbits? | quantum numbers |
| What does the quantum mechanical model assign? | principal quantum numbers (n) that indicate the relative sizes and energies of atomic orbitals |
| What does n specify? | the atom's major energy levels |
| What are the atom's major energy levels called? | the principle energy levels |
| What happens as n increases? | the orbital becomes larger, the electron spends more time farther from the nucleus, and the atom's energy increases |
| How many energy levels have been detected for the hydrogen atom? | Up to seven |
| How are sublevels labeled? | s,p,d,or f according to the shape of the atom's orbital. All s are spherical and all p are dumbbell |
| The maximum number of orbitals related to each principal energy level equals | n squared |
| Because each orbital may contain at most two electrons, the maximum number of electrons related to eac principal energy level equals | 2n squared |
| How can a hydrogen atoms have so many energy levels, sublevels, and related atomic orbitals? | At any given time, the atom's electron can occupy just one orbital |
| How many maximum electrons does each orbit contain? | A maximum of two electrons |
| What do we call the arrangement of electrons in an atom? | the atom's electron configuration |
| What arrangement do atoms tend to assume? | the one that gives the atom the lowest possible energy |
| What is the most stable, lowest-energy arrangement of the electrons in atoms of each element? | the element's ground-state electron configuration |
| This prinicipal states that each electron occupies the lowest energy orbital available? | the aufbau principle |
| In the aufbau diagram, what does each box represent? | an atomic orbital |
| All orbitals related to an energy level are of equal | energy.. all three 2p orbitals are of equal energy |
| In a multi-electron atom, the energy sublevels within a principal energy level have different | energies...the three 2p orbitals are of higher energy than the 2s orbital |
| In order of increasing energy, the sequence of energy sublevels within a principal energy level is | s,p,d,f |
| Orbitals related to energy sublevels within one principle energy level can overlap orbitals related to energy sublevels within another | principal level |
| States that a maximum of two electrons may ocupy a single atomic orbital but only if the electrons have opposite spins | The Pauli Exclusion Principle |
| An atomic orbital containing paired electrons with opposite spins is written as | (up arrow)(down arrow) |
| States that single electrons with the same spin must occupy each equal energy orbital before additional electrons with opposite spins can occupy the same orbitals | Hand's rule |
| A way of representing an electron's configuration by drawing a box for each of the atom's orbitals | orbital diagram |
| What does an empty box represent? | An unoccupied orbital |
| What does a box containing a single arrow represent? | an orbitral with one electron |
| What does a box containing both up and down arrows represent? | a filled orbital |
| What is the orbital diagram for a ground-state carbon atom which contains two electrons in the 1s orbital, two electrons in the 2s orbital and 1 electron in two of three separate 2p orbitals? | c (1s:up,down) (2s: up, down) (2p:up)(2p:up)(2p:empty box) |
| How many electrons does carbon (atomic number of 6 have)? | 6--number of electrons=number of protons |
| Another method of describing the arrangement of electrons in an element's atom by designating the principal energy level and energy sublevelassociated with each of the atom's orbital and including a superscript representing the number of electrons in each orbital is called... | electron configuration notation |
| Noble gas notation is a method of representing noble gases using | bracketed symbols |
| Electrons in the atom's outermost orbitals, those generally associated with the atom's highest principal energy level which determine the chemical properties of an element | valence electrons |
| simple shorthand method of writing valence electrons by using dots | electron-dot structure |
