| A | B |
|---|
| VALENCE ELECTRONS | ELECTRONS FOUND IN THE OUTER |
| ENERGY LEVEL | any of the poissible energies an electron may have in an atome |
| ORBITAL | A region in an atom where there is a high probability of finding electrons |
| DIATOMIC | pure elements that form molecules consisting of two atoms bonded together |
| LEWIS STRUCTURE | drawing of a molecule that illustrates the valence electrons for the element |
| ELECTRON CLOUD | current theory or model of the atom where electrons move three dimensionally within a given area |
| SUBSCRIPT | written in a chemical formula to communicate number of atoms of element in compound |
| CATION | result of an element changing from neutral state to positive because the element gave up electrons |
| ANION | result of an element changing from neutral state to negative as a result of gaining electrons |
| ION | charged particle as a result of losing or gaining electrons |
| OXIDATION NUMBER | charge that atom would have if the compound was composed of ions |
| SUPERSCRIPT | SYMBOLIZES THE OXIDATION NUMBER OF AN ELEMENT |
| SUBSCRIPT | numbers that come after a symbol and below, tell you the number of. atoms of that element |
| 1 | number of atoms if element does not have a subscript |
| VALENCE ELECTRONS | ELECTRONS FOUND IN THE OUTER |
| ENERGY LEVEL | any of the poissible energies an electron may have in an atome |
| ORBITAL | A region in an atom where there is a high probability of finding electrons |
| LEWIS STRUCTURE | drawing of a molecule that illustrates the valence electrons for the element |
| ELECTRON CLOUD | current theory or model of the atom where electrons move three dimensionally within a given area |
| CATION | result of an element changing from neutral state to positive because the element gave up electrons |
| ANION | result of an element changing from neutral state to negative as a result of gaining electrons |
| ION | charged particle as a result of losing or gaining electrons |
| CORE ELECTRONS | electrons that are NOT in the outer orbital/shell of the atom |
| OCTET RULE | max of eight valence electrons; full outer shell |
| 3rd orbital or energy level | M shell |
| ELECTRONEGATIVITY | The ability for an atom to attract electron. |
| 6 | number of valence electrons for oxygen |
| single bond | A chemical bond formed when atoms share one pair of electrons. |
| double bond | A chemical bond formed when atoms share two pairs of electrons. |
| polar bond | A covalent bond in which electrons are shared unequally. |
| non-polar bond | A covalent bond in which electrons are shared equally. |
| number of orbitals | Period number is equal to ________ |
| decreases | Ionization energy _____ as you move down a group on the periodic table |
| valence electrons | Elements in the same group have the same number of _____. |
| It increases because the electron number goes up | The amount of energy needed to remove an electron ____ from left to right across a period. |
| 2 electrons | Alkaline earth metals lose _____ electrons to achieve the electron configuration of the noble gas in the preceding period. |
| an electron | Ionization energy is the energy required to remove ____ from an atom of an element. |
| covalent bond | occurs when pairs of electrons are shared by atoms |
| ionic bond | attraction between oppositely charged ions in a chemical compound |
| COVALENT BOND | -intermolecular interaction between non-metals (small difference in electronegavity) -equal sharing of electrons between the non-metals |
| IONIC BOND | - metal and nonmetal - metal donates electrons = CATION - nonmetal accepts electrons = ANION |
| HYDROGEN BOND | a weak bond between two molecules resulting from an electrostatic attraction between a proton in one molecule and an electronegative atom in the other. |
| POLAR COVALENT BOND | Is a particular type of covalent bond. It is formed between two atoms where the electrons forming the bond are unequally shared, and therefore, unequally distributed. |
| NON POLAR COVALENT BOND | Is a particular type of covalent bond. It is formed between two atoms where the electrons forming the bond are equally shared, and therefore, equally distributed. |
| METALLIC BOND | A bond between metals. |
| VALENCE ELECTRONS | The electrons in the outermost shell in an atom. |
| COVALENT BONDS | A bond formed by atoms SHARING electrons. |
| ELECTRONEGATIVITY | The ability of an atom to attract shared electrons |
| IONIC BOND | A bond formed by the TRANSFER of electrons from one atom to another |
| POLAR COVALENT BOND | Bonds with partially covalent and partially ionic are called... |
| NON POLAR COVALENT BOND | Formed by the equal (or nearly equal) sharing of electrons between two nonmetal metalloid atoms |
| POLAR COVALENT BOND | What type of bond is in H2O |
| IONIC BOND | Formed by the transfer of electrons from a metal to a nonmetal |
| POLAR COVALENT BOND | Formed by uneven sharing of electrons between two nonmetals or metalloids |
| METALLIC BOND | What type of bond is in FeTi |
| IONIC BOND | What type of bond is in NaCl |
| VALENCE ELECTRONS | ELECTRONS FOUND IN THE OUTER |
| ENERGY LEVEL | any of the poissible energies an electron may have in an atome |
| ORBITAL | A region in an atom where there is a high probability of finding electrons |
| SUBSCRIPT | written in a chemical formula to communicate number of atoms of element in compound |
| CORE ELECTRONS | electrons that are NOT in the outer orbital/shell of the atom |
| OCTET RULE | max of eight valence electrons; full outer shell |
