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Chem Exam Review
| Term | Definition |
|---|---|
| Explain the mathematical relationship between the wavelength, frequency, and energy of electromagnetic radiation. | Frequency and wavelength are inversely proportional. This means that while one increases the other decreases. Energy is directly proportional and inversely proportional to wavelength. |
| How are the colors on the visible spectrum (ROY-G-BIV) relating to the energy levels of the atoms? | Colors that are visible to this spectrum relate to the energy levels of atoms because they represent different amounts of energy that are carried out by photons.This causes the electrons to jump between different levels of energy. |
| Why can the same types of atoms be producing the different colors of closely spaced lines in the spectrum? What do these lines in the spectrum prove? | The electron at the same ground state can be excited to different higher energy levels (different excited states) depending on the amount of energy absorbed by the electron. The closely spaced lines in the spectrum with different colors show |
| When does an electron emit energy and absorb energy? | Electron absorbed energy when excited and move from ground state/lower energy level to higher.Excited electron is unstable at higher energy and will emit photons (quantum energy) & moves from excited state back to ground state/Higher energy back to lower. |
| What are an absorption spectrum? | An absorption spectrum is the missing lines on the visible spectrum, showing the quanta energy that are absorbed by the electron.lines on Absorption & emission spectrum are same bc electron will emit the same quanta energy that was absorbed. |
| State Heisenberg’s uncertainty principle and what has this discovery led to? | It concluded that it is impossible to measure accurately both the position and the energy of an electron at the same time. This discovery led to the electron cloud model or quantum model because Bohr’s “planetary” model is no longer true. |
| What is the principal quantum number represent 1s2? | The principal quantum number “n” represents the main energy level, same as the rows or the period numbers on the periodic table. |
| electron configuration of Potassium | 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 or [Ar] 4s 1 |
| electron configuration of oxygen | 1s 2 2s 2 2p 4 or [He] 2s 2 2p 4 |
| List the four sublevels in the atoms. | s,p,d,f |
| What are the sublevels also known as? | They are also known as orbitals or electron cloud. |
| What is an emission spectrum? | An emission spectrum is the colored lines showing the quanta energy that are emitted by the electron. |
| What are the shapes of each type of these sublevels? | s = spherical p = dumbbell d = four-leaves clover f = very complex |
| How many orbitals are of the same type of sublevels. | s = 1 p = 3 d = 5 f = 7 |
| What are the maximum numbers of electrons that can occupy each type of these sublevels? | s = 2 p = 6 d = 10 f = 14 |
| How are these sublevels represented in the periodic table? | s = Group 1 and 2 p = Group 13 to 18 d = Group 3 to 12 f = Inner transition metals |
| What is electron configuration? | Electron configuration is the way to show the location of every electron in the atom. |
| What are the coefficient and superscript stand for?(electron Configuration) | Coefficient = main energy level and Superscript = numbers of electrons |
| How is the electron configuration arranged? | electron config. arranged distance from nucleus,increasing energy lvl or energy possessed by electron: Closer to the nuc. = lower energy lvl = less energy is possessed by e- Further from the nuc. = higher energy lvl = more energy is possessed by the e- |
| What are valence electrons? Know how to find the numbers of valence electrons. | They are the outermost electrons or at the highest energy levels within known atom. These are the electrons that are being gained, lost, or shared during the chemical bondings.They are found in the “s” or “s and p” |
| electromagnetic radiation | a form of energy that exhibits wavelike behavior as it travels through space. |
| wavelength | represented by the Greek letter lambda - is the shortest distance between equivalent points on a continuous wave. |
| frequency | represented by the Greek letter nu - the number of waves that pass a given point per second. |
| amplitude | the wave’s height from the origin to a crest, or from the origin to a trough. |
| electromagnetic spectrum | encompasses all forms of electromagnetic radiation, with the only differences in the types of radiation being their frequencies and wavelengths. |
| quantum | the minimum amount of energy that can be gained or lost by an atom. |
| line emission spectrum | the set of frequencies of the electromagnetic waves emitted by atoms of the element. |
| ground state | the lowest allowable energy state of an atom. |
| continue spectrum | the emission of a continuous range of frequencies of electromagnetic radiation |
| excited state | a state in which an atom has a higher potential energy than it has in its ground state. |
| photon | a particle of electromagnetic radiation having zero mass and carrying a quantum of energy |
| Heisenberg uncertainty principle | states that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time. |
| orbital | a three-dimensional region around the nucleus called an describes the electron’s probable location. |
| principal quantum numbers | symbolized by n, indicates the relative sizes and energy level occupied by the electron. |
| Hunds Rule | Describes how electrons are distributed among orbitals of the same sublevel when there is more than one way to distribute them.Electrons will only pair up in an orbital when all orbitals in the same sublevel have one electron. |
| The Aufbau Principle | filling atomic orbitals with electrons in order of increasing energy, starting with the lowest energy orbitals |
| The Pauli Exclusion Principle | Describes the restriction the placement of electrons into the same orbital.If two electrons occupy the same orbital they must have opposite spins |
| True/False:The Configuration [He] 2s^2 2p^4 is an abbreviated form of the configuration 1s^2 2s^2 2p^4 | True |
| True/False:The max number of electrons in any p sublevel is three | False |
| True/False:The lower frequency of electromagnetic radiation,the shorter its wavelength is | False |
| True/False: When an electron absorbs a specific amount of energy,the electron can jump to a higher energy level | True |
| True/False:The 1s Orbital is farther from the nucleus than is the 2s sublevel | False |
| True/False:In general, the closer an orbital is to the nucleus,the more energy an electron possesses | False |
| True/False:All s orbitals are Spherical | True |
| True/False:In moving from a higher energy level to a lover energy level in an atom,an electron emits energy | True |
| True/False:The symbol {He} stands for the electron configuration 1s^2 2s^2 | False |
| True/False:The designations used to represent electron energy sublevels in an atom are x,y,z | False |
| Short Answer:From its position in the periodic table,write the electron configuration of each element. Use noble core abbreviations if necessary | Bromine: [Ar] 4s^2 3d^10 4p^5 Cadmium: [Kr] 5s^2 4d^10 Nitrogen:1s^2 2s^2 2p^3 or [He] 2s^2 2p^6 |
| Briefly explain why each electron configuration is inncorrect arrangment:1s^2 2s^2 p^6 3s^2 | Electron configuration is incorrect bc it skips the 2p subshell. |
| An atom is in Group 2,Period 3. How many electrons does the atom contain? a.2 b.3 c.6 d.12 | 12 |
| A p orbital has a...shape a.spherical b.dougnout c.dumbshell d.four leaf clover | Dumbshell |
| Match terms: a.1s^2 2s^2 2p^6 3s^2 2p^6 b.Ianthanide/actinide c.can hold max of 2 elec. d.discov. led to elec. cloud mod. e. s,p,d, or f within ener. lvl 1:orbit. 2:sublvl 3:elec. config. 4;Inner transit. elem. 5:Heisenberg uncertainty princ. | 1:c-orbutal 2:e-sublevel 3:a-electron configuration 4;b-inner transition element 5:d-Heisenberg uncertainty principle |
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