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Unit 3
Chemistry
| Question | Answer |
|---|---|
| Define electromagnetic spectrum. | Arrangement of different types of electromagnetic radiation from longest wavelength to shortest wavelength. |
| What are the ranges of the electromagnetic spectrum? | It ranges from radio waves to gamma rays. Radio waves have the longest wavelength and least energy while gamma rays have the shortest wavelength and highest energy. |
| The longest wavelength has ________? | The lowest frequency. |
| Waves with the shortest wavelength have_________? | The highest frequency. |
| How are wavelength and frequency related? | They are inversely related. |
| Describe the Bohr model of Hydrogen Atom. | An electron circles the nucleus only in fixed energy ranges called orbits. An electron can neither gain or lose energy inside this orbit, but could move up and down to another orbit. |
| Describe Line Emission Spectrum. | If the energy that is emitted (from the Bohr model) is visible, then we see one of the colors of visible light. When electricity is passed through a sample of gas, the atoms produce a spectrum of a few parallel lines. |
| Describe Schrodinger-Quantum Mechanical Model relectron cloud model. | It does not define the exact path of an electron like the Bohr model does. Dense regions are known as "electron orbitals", since they are the most likely location where an orbiting electron will be found. |
| In the Schrodinger Model, where is the greatest probability the electron will be found? | Where the cloud is most dense, when its less dense it becomes less likely. |
| Define electron energy levels. | In an atom, each electron has a specific energy levels, each level has a maximum number of electrons using the formula 2n^2. |
| In energy level 1, what is the max number of electrons? | 2 |
| In energy level 2, what is the max number of electrons? | 8 |
| In energy level 3, what is the max number of electrons? | 18 |
| In energy level 4, what is the max number of electrons? | 32 |
| Describe electrons in the lower and higher levels. | The lower energy level are closest to the nucleus and those in higher energy levels are further away. |
| What are the sublevels? | S, P, D, and F |
| What is the order of the sublevels? | S<P<D<F |
| Define orbitals. | Is a 3-dimensional volume in which electrons have the highest probability of being found. No way to determine the location of one electron. |
| What is the S sublevel orbital? | Up to 2e- |
| What is the P sublevel orbital? | Up to 6e- |
| What is the D sublevel orbital? | Up to 10e- |
| What is the F sublevel orbital? | Up to 14e- |
| Mnemonic device to remember all the sublevels...? | S-spherical P-peanut D-double peanut F-flower |
| What gas cannot abbreviate themselves? | Noble gases. |
| How to write electron configurations? | Put the element in brackets and then write the 1s^2 part. (1s^2 is just an example). |
| What is pauli's exclusion principle? | An electrons is spinning on its axis which generates a magnetic field. 2 electrons are in the same orbit, the repel each other. Must have opposite spins. |
| What is hund's rule? | For orbitals of equal energy, one e- enters each orbital unit all orbitals contain 1 e- before pairing. (the arrows) |
| What is aufbua principle? | E- enter orbitals of lowest energy first. Orbitals of a sublevel are equal energy (s sublevel is lowest). |
| In s sublevel, how many electrons? | 2 |
| In p sublevels, how many electrons? | 6 |
| In d sublevel, how many electrons? | 10 |
| In d sublevel, how many electrons? | 14 |
| Define valence electrons. | Electrons in the outermost energy level, Occupy the S and P sublevels with the highest principle quantum number. |
| Define atomic radius. | Is determined by the distance of the valence electrons from the nucleus. |
| Define electron shielding effect. | When electrons are in multiple energy levels, electrons in the lower levels "shield" the outer electrons from the pull of the protons. |
| What are the trends in atomic radius? | Increases from top to bottom in a group and decreases across a period. (left to right) |
| What are the trends in metallic character? | Decreases let to right across a period and increases from top to bottom in a group. |
| Define ions. | Is an atom that has a positive or negative charge. Formed when electrons are transferred between atoms. |
| Define cation. | Atom loses one or more electrons, charge is positive, and size is smaller. |
| Define anion. | Atom gains one or more electrons, charge is negative, and size is larger. The more negative the bigger the ion. |
Created by:
CoraEvelynnBaker
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