1600481
Description
Flashcards by Hannah Goodenough, updated more than 1 year ago
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Created by Hannah Goodenough
about 10 years ago
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| Question | Answer |
| Plasma | A mixture of positive and negative electrons. |
| First ionisation energy (1st I.E) | Is the energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions. |
| What is the first ionisation energy of Sodium? | Na(g) ----> Na+(g) + e- |
| Factors affecting ionisation energy: | *Atomic Radius *Nuclear Charge *Electron shielding |
| The greater the atomic radius... | The smaller the nuclear attraction experienced by outer electrons. |
| The greater the nuclear charge... | The greater the attractive force on the outer electrons. |
| Electronic Shielding | Is the repulsion between electrons in different inner shells. Shielding reduces the net attractive force from the positive nucleus on the outer-shell electrons. |
| The more inner shells... | *The larger the electronic shielding *The smaller the nuclear attraction experienced by outer electrons. |
| Successive ionisation energies | Are a measure of the energy required to remove each electron in turn. |
| Second ionisation energy | Is the energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions. |
| What is the second ionisation energy of Lithium? | Li+(g) --> Li2+(g) + e- |
| Evidence for shells | Successive ionisation energies. |
| Shell | Is a group of atomic orbitals with the same principal quantum number, n. |
| Principle quantum number (n) | Is a number representing the relative overall energy of each orbital, which increases with distance from the nucleus. |
| Atomic orbital | Is a region within an atom that can hold up to two electrons, with opposite spins. |
| What's the formula for how many electrons each shell holds? | 2n squared |
| How many electrons in shell.. *1 *2 *3 *4 | Shell 1 has 2 electrons. Shell 2 has 8 electrons. Shell 3 has 18 electrons. Shell 4 has 32 electrons. |
| What shape is a s-orbital? | Spherical shape. |
| What shape is a p-orbital? | Dumb-bell shape. |
| How many s-orbitals in one shell? | One s-orbital per shell. |
| How many p-orbitals in one shell? | Three p-orbitals per shell. |
| How many d-orbitals in one shell? | Five d-orbitals per shell. |
| How many f-orbitals in one shell? | Seven f-orbitals per shell. |
| Sub-shell | Is a group of the same type of atomic orbitals (s,p,d or f) within a shell. |
| What is the order of sub-shells by energy level from smallest to largest? | 1s,2s,2p,3s,3p,4s,3d,4p,4d,4f |
| Electron configuration | The arrangement of electrons in an atom. |
| What is the Aufbau principle? | *Electrons are added, one at a time, to 'build up' the atom. *The lowest available energy level is filled first. *Each energy level must be full before the next higher energy level. *Each orbital is filled singly before pairing starts. |
| What is the electron configuration of Oxygen? | 1s(2),2s(2), 2p(4). |
| When positive ions are formed, electrons are... | removed from the highest energy orbital. |
| When negative ions are formed, electrons are... | Added to the highest energy orbital. |
| What group in the periodic table have elements that are naturally single unbonded atoms? | Group 0 (The noble gases) |
| Octet Rule | The tendency for atoms to combine to acquire a noble gas configuration. (8 electrons in their outer shell) |
| Compound | Is a substance formed from two or more chemically bonded elements in a fixed ratio, usually shown by a chemical formula. |
| What compounds do ionic bonds occur in? | Metal and non metal compounds. (Electrons are transferred from the metal atom to the non-metal) |
| What compounds do covalent bonds occur in? | Two non metals. (electrons are shared between the atoms) |
| Where do metallic bonds occur? | In metals. (electrons shared between all atoms) |
| What is Krypton used in? | Lasers for eye surgery. |
| What is Argon used in? | Filament light bulbs. |
| What is Helium used in? | Airships. |
| What is Neon used in? | Advertising signs. |
| What is Xenon used in? | Car headlights. |
| Ionic bond | Is the electrostatic attraction between oppositely charged ions. |
| Giant ionic lattice | Is a three-dimensional structure of oppositely charged ions, held together by strong ionic bonds. Eg. NaCl. |
| A group | Is a vertical column in the Periodic Table. Elements in the same group have similar chemical properties and their atoms have the same number of outer-shell electrons. |
| What is the overall charge of an ionic compound? | Zero. |
| What are the charges of: *NO3 *CO3 *SO4 *NH4 | *(NO3)- *(CO3)2- *(SO4)2- *(NH4)+ |
| Covalent bond | Is a bond formed by a shared pair of electrons. |
| How many covalent bonds do the following atoms of these elements form? C,N,O,H | C: 4 covalent bonds N: 3 covalent bonds O: 2 covalent bonds H: 1 covalent bond |
| Lone pair | Is an outer-shell pair of electrons that is not involved in chemical bonding. |
| The sharing of two pairs of electrons forms... | A double bond. eg. O=O |
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