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30 Cards in this Set
- Front
- Back
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Period |
The outer most shell being filled |
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Group |
The number of electrons in the valence shell of an electron |
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Ionisation energy |
The amount of energy that isrequired to remove an electron from an atom.*First Ionisation energy is energy required to removeoutermost electron |
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Electronegativity |
Electron attracting power |
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Periodic table trends: Group |
Metallic nature (increases) Atomic size (increases) Electronegativity (decreases) Ionisation energy (decreases) |
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Periodic table trends: Period |
Metallic nature (decreases) Atomic size (decreases) Electronegativity (increases) Ionisation energy (increases) |
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Element |
A substance made from only one type ofatom that can not be broken down by chemicalmeans. |
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Compounds |
A substance formed when two ormore elements chemically bond together. |
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Electron |
A negatively charged subatomic particleorbiting the nucleus of an atom in electron shells. |
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Proton |
A positively charged subatomic particlefound in the nucleus of an atom. |
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Neutron |
A neutrally charge subatomic particlefound in the nucleus of an atom. |
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Mass number |
The number of protons and neutrons found in the atoms nucleus |
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Atomic number |
Determined by the number of protons an atom has |
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Electron shell configuration and rule |
The general arrangement for the elements 2, 8, 18, 36 (2n)squared |
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Features of a metal element |
-Located on the left side of the periodic table -Most shiny solids at room temperature -High MP and density -Low electronegativity and ionisation energy -Maleable -Metals usually form cations (lose electrons) |
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Features of a non-metal element |
-Located on the upper right hand side of the periodictable -Usually have fewer than 4 electron in outer shell-Solid or gas as room temp -Brittle -High Ionisation energy and electronegativity -Poor Electrical conductors -Non-metals usually for anions (gain electrons) |
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Mendeleev |
Organised the known elements into atable based on atomic mass and chemicalproperties. |
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Rutherford |
Conducted the gold foil experimentwhich led to the discovery that: -atoms had space -a small solid, positively charged nucleus -electrons surround the nucleus leaving lots ofnegative space |
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James Chadwick |
Discovered the neutron - asubatomic particle with mass but no charge. |
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J.J Thompson & Bohr |
Found discrete levels called shells |
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Ionic Bonding |
Transfer of electrons between metal(s)and non-metal(s)
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Anion |
Negatively charged ion (formed from nonmetals) |
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Cation |
Positively charged ion (formed from metals) |
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Meaning of Ide Ite Ate |
Ide=no oxygen Ite= 1 less oxygen than ate Ate= Maximum amount of oxygen |
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Polyatomic ions |
An ion composed of two or more atoms covalently bonded |
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List 3 ionic properties |
-High melting point -Solid -Don't conduct electricity (in solid state) |
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Covalent bonding |
The sharing of electrons between two non-metal atoms
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List the pre-words used to name the covalent compounds |
Mono: 1 Di: 2 Tri: 3 Tetra: 4 Penta: 5 |
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What is NO2 N2O SO3 |
Nitrogen monoxide Dinitrogen Monoxide Sulfur Trioxide |
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List the 5 reaction types and their equations |
Combustion Non-metal + Oxygen =CO2 + H2O Combination A+B=C Decomposition AB=A+B Single Replacement A+BC=AC+B Double Replacement AB+CD=AD+CB |
