Stallman 1
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100 terms
Terms | Definitions |
|---|---|
 Who discovered the electron? | Thomson |
| Who developed the billard ball model of the atom? | Dalton |
| Who did the cathode ray experiment? | Thomson |
| What did the cathode ray experiment help Thomson discover? | the electron |
| Who did the gold foil experiment? | Rutherford |
| What did Rutherford discover through the gold foil experiment? | that there was a positive nucleus, and that the atom was mostly empty space |
| Who created the planetary model of the atom? | Bohr |
| Isotopes are elements of the same atom, with a different number of ________. | neutrons |
| What is the difference between an atom and an ion? | Atoms have a charge of zero, Ions have a positive or negative charge. |
| Atoms have the same number of _________ as _________. | protons, electrons |
| Ions have a different number of ________ than protons | electrons |
| What is the formula for average atomic mass? | (mass#)(%) + (mass #)(%) + (mass #)(%) / 100 |
| How do you find mass #? | add protons + neutrons |
| How do you find number of neutrons? | Mass# - protons |
| How do you find number of protons? | protons are always found on the periodic table, and are the same as the atomic number |
| If an ion has a +4 charge and 20 electrons, how many protons would it have? | 24 |
| If an ion has a +4 charge and 20 protons, how many electrons would it have? | 16 |
| If an ion has a -2 charge and 30 electrons, how many protons would it have? | 28 |
| If an ion has a -2 charge and 30 protons, how many electrons would it have? | 32 |
| In isotope notation, what does the number up top represent? | mass number |
| In isotope notation, what does the number at the bottom represent? | atomic number (or number of protons) |
| An atom has 8protons, 11 neutrons, and 8 electrons. What is its mass number? | 19 |
| An atom has 10 electrons and a mass number of 22. How many neutrons does it have? | 12 |
| Name all the types of waves in the electromagnetic spectrum in order from longest wavelength to shortest wavelength. | radio, micro, Infrared, visible, Ultraviolet, x-ray, gamma |
| Which has higher energy, Infrared or Ultraviolet radiation? | Ultraviolet |
| What color has the highest energy? | violet |
| What color has the lowest energy | red |
| What color has the longest wavelength? | red |
| what color has the shortest wavelength | violet |
| What is the relationship between frequency and wavelength? | As wavelength decreases, frequency increases |
| What is the relationship between energy and wavelength? | As wavelength increases, energy decreases |
| What is the relationship between energy and frequency? | As energy increases, frequency increases |
| The shortest wavelength of the electromagnetic spectrum is _______. | gamma waves |
| The lowest energy wave of the electromagnetic spectrum is _______. | radio waves |
| When electrons make a quantum leap towards the nucleus, energy is _________. | emitted (given off) |
| When electrons make a quantum leap away from the nucleus, energy is __________. | absorbed |
| The lowest energy level is called the ______________. | ground state |
| When an electron gains energy and moves to a higher energy level, it is said to be in a(n) _______________. | excited state |
| What is the formula for calculating the wavelength of a visible wave? | λ = C/v |
| What is the formula for calculating the energy of a partiuclar wave? | E = hv |
| What is frequency commonly measured in? | Hz |
| What is the unit for Energy? | J |
| When an electron leaps to lower energy levels, it gives off colors. These colors act as a "finger print" and are called _____________________. | bright line spectras |
| Electromagnetic waves differ from mechanical waves in that they can travel through __________. | a vacuum (do not require matter to be present) |
| The speed of visible waves of light is | 3.0 x 10^8 m/s |
| The speed of a radio wave is | 3.0 x 10^8 m/s |
| Who created the wave equation? | Schroedinger |
| What quantum numbers make up the wave equation? | n, l, m, s |
| What does the quantum number "n" represent? | Principle quantum number (Energy level) |
| What does the quantum number "l" represent? | sublevel (shape) |
| What are the four possible sublevels? | s, p, d, f |
| What shape is the "s" sublevel? | sphere |
| What shape is the "p" sublevel? | dumbell |
| What shape is the "d" sublevel? | x-shaped |
| What shape is the "f" sublevel? | complex shape |
| What does the quantum nubmer "m" represent? | magnetic quantum number, or # of orbital arrangements |
| The "s" sublevel has _______ orbital arrangements. | 1 |
| The "p" sublevel has _________ orbital arrangements. | 3 |
| The "d" sublevel has _________ orbital arrangements. | 5 |
| The "f" sublevel has _________ orbital arrangements. | 7 |
| What does the quantum number "s" represent? | spin of the electron |
| How many electrons can fit into each orbital? | 2 |
| How many electrons can possibly fit inside any "p" sublevel? | 6 |
| How many electrons can possibly fit inside any "s" sublevel? | 2 |
| How many electrons can possibly fit inside any "d" sublevel? | 10 |
| How many electrons can possibly fit inside any "f" sublevel? | 14 |
| How many electrons can fit in n1? | 2 |
| How many electrons can fit in n2? | 8 |
| How many electrons can fit in n3? | 18 |
| What do the rows on the periodic table represent? | The energy level (n) |
| When writing shorthand notation, what group on the periodic table do you use? | Group 18 - the noble gasses |
| According to the Aufbau principle, which energy level would you fill first, 3s, 3d, 4s, 3p? | 3s |
| How many valence electrons would Calcium have? | 2 |
| What are valence electrons? | electrons in the last energy level of an atom |
| How many unshared electrons would Argon have? | 0 |
| Heisenbergs uncertainty principle states that _____________. | The position and momentum of an electron cannot be measured and known exactly. |
| What is the current model of the atom? | Electron cloud model |
| What does the alpha particle look like? | 4He 2 |
| What does the beta particle look like? | 0e -1 |
| What does the K-capture particle look like? | 0e -1 |
| What does the positron particle look like? | 0e +1 |
| What does the neutron particle look like? | 1n 0 |
| What is the difference between alpha bombardment and alpha decay? | The alpha particle is on the right side of the equation for "decay" , and on the left side for "bombardment" |
| What is fission? | The breaking down of a nucleus into two smaller nuclei. |
| What is fusion? | the formation of a new more massive atom through the combination of 2 smaller nuclei. |
| The sun is an example of _________. | fusion |
| Which subatomic particle has the smallest mass? | electron |
| What is transmutation? | One element changing into another element by a nuclear change. |
| What is the electron configuration for Bromine? | 1s2 2s2 sp6 3s2 3p6 4s2 3d10 4p5 |
| What is the shorthand notation for Bromine? | [Ar]4s2 3d10 4p5 |
| How many valence electrons does Bromine have? | 7 |
| How many unshared electrons does Bromine have? | 1 |
| The number of protons will always be the same as the _______ _________. | atomic number |
| How many electrons can possibly fit in sublevel 3d? | 10 |
| How many total orbitals are in n2? | 4 |
| How many sublevel does n4 have, and what are they? | 4. s, p, d, f |
| What does hunds rule state? | When electrons enter orbitals of equal energy (same n,l), one electron enters each orbital until all the orbitals contain one electron with parallel spins, then they can pair up. |
| What does Pauli exculsion principle state? | an atomic orbital may contain at most 2 electrons |
| To calculate the maximum number of electrons for any energy level, you would use _______. | 2n^2 |
| Are you going to study? | YES!!! |
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