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Chemistry Unit 4
| Term | Definition |
|---|---|
| Describe Dalton's indivisible atom | hard, round, marble like solid mass |
| Describe Thomposon's atom | charged particles (proton, electron, neutron), plum pudding atom |
| Describe Rutherford's atom (gold foil experiment) | nuclear atom, mass in center (nucleus), mostly empty space |
| Describe Bohr's atom | planetary atom, electrons have a path that they follow, rungs of a ladder, different energy needed for quantum jumps/leaps |
| Quantum Mechanical atom | describes the behavior and energy of the electron in hydrogen, the path of an electron is not described |
| Schrodinger | used new knowledge to devise and solve a mathematical equation describing the behavior and energy of the electron |
| Probability maps (electron cloud) | volume in which the electron is found 90% of the time (rotating propeller, cannot know where it is at all times without changing it) |
| Atomic Orbital | region in which the electron is found, fixed path |
| Principle Quantum Number (principle energy level) | Each principle energy level has energy sublevels |
| 1 orbital- spherical | s |
| 3 orbitals- dumbell | p |
| 5 orbitals- clover/complex | d |
| 7 orbitals-complex | f |
| what is the lowest energy level | n=1 |
| Noble Gases | The far right column of the periodic table |
| Electrons orbit in specific... | energy levels or shells |
| How many energy levels are there? | seven |
| Each energy level is divided into | sublevels and orbitals |
| hertz | the SI unit of frequency |
| atomic orbital | a region outside the nucleus where there is high probability of finding an electron |
| spectrum | a range of colors seen when light passes through a prism |
| atomic emission spectrum | lines of colored light obtained by passing the light emitted by an element through a prism |
| quantum of energy | the amount of energy required to move an electron from one energy level to the next higher one |
| amplitude | the height of a wave from the origin to the crest |
| wavelength | the distance between crests of waves |
| energy level | the region around an atomic nucleus where an electron is likely to be moving |
| Aufbau principle | Electrons enter orbitals of lowest energy first |
| frequency | the number of wave cycles that pass a given point per unit of time |
| metal | good conductor of heat and electric current |
| halogen | any nonmetal in group 7A |
| inner transition metal | an element whose highest occupied s sublevel and a nearby f sublevel contain electrons |
| representative element | an element whose highest occupied s or p sublevels are partially filled |
| ionization energy | the energy needed to remove an electron from an atom in the gaseous state |
| alkaline earth metal | an element in Group 2A |
| cation | positively charged ion |
| electronegativity | the tendency of an atom to attract electrons when the atom is in a compound |
| transition metal | an element whose highest occupied s sublevel and a nearby d sublevel contain electrons |
| noble gas | an element in which the highest occupied s and p sublevels are filled |
| the fourth principle energy level has | 16 orbitals |
| If the electron configuration of an element is 1s22s2sp63s23p5 the element is... | chlorine |
| The quantum mechanical model of the atom | is concerned with the probability of finding an electron in a certain position |
| The electron configuration of calcium | 1s22s22p63s23p64s2 |
| The maximum number of electrons that can occupy the third principle level is | 18 |
| As the frequency of light increases, the wavelength | decreases |
| The formula 2n2 represents | the maximum number of electrons that can occupy an energy level |
| In order to occupy the same orbital, two electrons must have | opposite spin |
| Stable electron configurations are likely to contain | filled energy sublevels |
| According to Hund's rule, when electrons occupy orbitals of equal energy, one electron enters each orbit until | all the orbitals contain one electron, with spins parallel |
| In the periodic table, there is a periodic pattern in the physical and chemical propeties of elements when they are arranged in order of | increasing atomic number |
| Which sublevel corresponds to the transition metals on the periodic table | d |
| The representative elements are | Group A elements |
| Which of the following elements is a metalloid As Se Br Kr | As |
| When a strontium atom loses two electrons to form an Sr^2+ ion, the electrons are lost from the | 5s orbital |
| The element iodine is a | period 5 halogen |
| The subatomic particle that plays the greatest role in determining the physical and chemical properties of an element is the | electron |
| Which of the following atoms would you expect to have the largest atomic radius I K Ca Rb | Rb |
| From left to right across the second period of the periodic table first ionization energy increases atomic radii increase electronegativity decreases atomic mass decreases | first ionization energy increases |
| For which element would you expect a large jump between the first and second ionization energies? | Na |
| The category of elements that is characterized by the cilling of f orbitals is the | inner transition metals |
| Electronegativity generally... | decreases from top to bottom within a group |
| Atomic size generally... | decreases from left to right across a period |
| Of the following atoms, which one has the smallest first ionization energy boron aluminum nitrogen silicon | aluminum |
| The alkali metals do not include... Li Ca Na Rb | Ca |
| Daltons atom | indivisible, solid mass |
| Thompsons atom model | plum pudding model, proton +, electron- |
| Rutherfords model | Nuclear atom (nucleus), mass in center, mostly empty space |
| Bohrs model | planetary atom, electron energy levels, rungs of a ladder, different energy needed for quantum jumps/leaps |
| Quantum Mechanical Atom (Schrodiner) | path of electron not described |
| Atomic orbital | region in which the electron is found |
| Equation for # of orbitals | n^2 |
| Equation for # of electrons | 2n^2 |
| Rule #1 (Aufbau's principle) | fill in lowest energy orbital first |
| Rule #2 (Aufbau's principle) | Pauli exclusion principle, maximum of 2 electrons per orbital and they must have opposite spins |
| Rule #3 (Aufbau's principle) | Hund's rule- must have maximum number of unpaired electrons for equal energy orbitals. Fill one at a time. |
| Frequency | things occuring in a certain amount of time (v) |
| C=? | 3x10^8 m/s |
| what is plank's constant (h) | 6.6x10^-34 J-S |
| E= | hv |
| C= | wavelength x frequency |
| What part of the electromagnetic spectrum has the lowest energy? | Radio |
| What part of the electromagnetic spectrum has the highest energy? | Gamma Rays |
| Rank the parts of the electromagnetic spectrum from highest energy to lowest energy | Gamma Rays, X Ray, UV, ROYGBIV, I.R., microwaves, Radio |
| Rank the parts of the electromagnectic spectrum from lowest frequency to highest frequency? | Radio, microwaves, I.R., ROYGBIV, UV, X Ray, Gamma Rays |
| Rank the parts of the electromagnetic spectrum from shortest wavelength to longest | Gamma Rays, X Ray, UV, ROYGBIV, I.R., microwaves, Radio |
| What is the relationship between frequency and wavelength | The lower the frequency, the longer the wavelength |
| What is the relationship between frequency and energy | If the frequency is low, so is the energy |
| Electron returns to level 1- | ultraviolet |
| Electron returns to level 2- | visible |
| Electron returns to level 3- | infrared |
| Photons | bundles of energy |
| Photoelectrons | the emitted electron |
| Threshold concept | amount of energy needed to emit the electron |
| more energy = | higher chance electron gets emitted |
| What element ends in the electron configuration 5d9 | Au |
| How many sublevels are ther in quantum level 4 | 4) s,p,d,f |
| In the hydrogen atom, an electron that jumps from quantum level 6 to quantum level 2 would be found in what portion of the electromagnetic spectrum? | visible |
| Which color has the greatest frequency? | violet |
| Moving across a period, Atomic Size | decreases |
| Moving down a group, atomic size | increases |
| Moving across a period, ionization energy | increases |
| moving down a group, ionization energy | decreases |
| moving across a period, electronegativity | increases |
| moving down a group, electronegativity | decreases |
| Ionization energy | the energy to remove an electron |
| Electronegativity | A measurement of how well an atom pulls in an electron |
| FONClBrISCH | commonly compared elements with electronegativity |
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