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Atomic structure
vocab 2
| Term | Definition |
|---|---|
| Group | Each vertical column of the periodic table. Atoms in the same group have similar properties because they have the same number of valence electrons |
| Period | Each horizontal row of the periodic table |
| Atom | The smallest particle of an element that retains its identity in a chemical reaction. Means charge is neutral, protons=electron |
| Atomic Mass | The weighted average mass of the atom in a naturally occurring sample of the element. This is always a decimal because it is a weighted AVERAGE of mass numbers. |
| Atomic Number | The number of protons in the nucleus of an atom of that element. This determines the identity of the element, this is the basic of the periodic table, this determined the nuclear charge. |
| Electron | Negatively charged subatomic particles. These have no mass and a charge of -1 |
| Isotopes | Atoms that have the same number of protons but different numbers of neutrons. The different number of neutrons give isotopes different mass numbers. |
| Mass number | The total number of protons and neutrons in an atom. Must be a whole number because protons and neutrons weigh whole numbers, this is the number of nucleons |
| Nucleon | The particles in the nucleus of an atom, this is the total of the protons and neutrons in an atom, equal to mass number |
| Nuclear charge | The charge of the nucleus of an atom, this is always positive and equals the number of protons |
| Neutron | Subatomic particles with no charge but mass nearly equal to that of a proton |
| Nucleus | The tiny central core of an atom and is composed of protons. Discovered by Gold Foil Experiment, contains all the mass of an atom, has a positive nuclear charge |
| Proton | Positively charged subatomic particles. Has a mass of 1 AMU and a charge of +1, determines the nuclear charge of an element, is the atomic number of an element, determines the identity of an atom |
| Atomic Emission Spectrum | The wavelength of the spectral lines are characteristic of an element. The atomic emission (or bright line) spectrum is emitted when an electron falls from a higher to lower energy level |
| Atomic Orbital | The probability of finding an electron at various locations around the nucleus |
| Excited State | When an electron absorbs energy, it moves to a higher energy level than normal |
| Ground State | When the electron has its lowest possible energy |
| Alkali Metals | The elements in Group 1 |
| Alkaline Earth Metals | The elements in Group 2 |
| Anion | An ion with a negative charge |
| Atomic Radius | One half of the distance between the nuclei of two atoms of the same element when the atoms are joined |
| Cation | An ion with a positive charge |
| Electronegativity | The ability of an atom of an element to attract electrons when the atom is a compound |
| Halogens | The non-metals in Group 17 |
| Ion | An atom or group of atoms that has a positive or negative charge. Number of protons and neutrons are NOT equal. |
| Ionization Energy | The energy required to remove an electron from an atom |
| Metalloids | Has properties that are similar to metals and non-metals |
| Metals | Good conductors of heat and electric current |
| Noble Gases | The elements in Group 18 |
| Non-metals | Poor conductors of heat and electric current |
| Transition metals | Element in groups 3-12 on the periodic table, known for making very colorful compounds and solutions |
Created by:
abbeebrandow
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