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Chemistry ch. 7
| Term | Definition |
|---|---|
| atomic radius (covalent radius) | half the distance between the nuclei of two atoms of the same element that are joined together by a single covalent bond |
| The values of atomic radius increase down any one group in the periodic table for two reasons: | 1. additional electrons are going into a new shell which is further from the nucleus. 2.Screening effect: inner shells of electrons help shield the outer electrons from the attractive force of the increasing nuclear charge. |
| The values of atomic radius decrease from left to right across a period in the periodic table for two reasons: | 1. increasing nuclear charge. 2. no increase in the screening effect.(electron being added is going into the same outer shell) |
| First ionisation energy | the energy required to completely remove the most loosely bound electron from a neutral gaseous atom. |
| the values of ionisation energy decrease down the groups in the periodic table for two reasons: | 1. increasing atomic radius:outermost electrons are further away from the attractive force of the nucleus and are more easily removed. 2. Screening effect of inner electrons: outermost electrons are shielded from the attractive power of the nucleus |
| The values of ionisation energy increase across the periods in the peroiodic table for two reasons: | 1. increasing nuclear charge: electrons are being held more firmly- require more energy to remove 2. decreasing atomic radius: outermost electrons are closer to the attractive power of the nucleus and are harder to remove |
| the values of electronegativity decrease down the groups in the periodic table for two reasons: | 1. increasing atomic radius: smaller attraction between the nucleus and the shared pair of electrons. 2. screening effect of inner electrons: outermost electrons (involved in bonding) are shielded by the attraction of the nucleus. |
| the values in electronegativity increase across the periods in the periodic table for two reasons: | 1. increasing nuclear charge: attraction between the nucleus and the outer electrons is increasing. 2. decreasing atomic radius: electrons in the outermost level are closer to the nucleus - greater force of attraction |
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sophielil
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