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5B Periodic Trends
| Question | Answer |
|---|---|
| Atomic Radius | Atomic radius is defined as half the distance between the nuclei of atoms of the same element that are joined by a single covalent bond. |
| Trends in Atomic Radius going down a group. 2 reasons | Atomic radius INCREASES. 1: A new shell is being added as we move down the table. 2: The screening effect of the extra electrons cancels out the pull of the growing nucleus. |
| Trends in Atomic Radius going left to right across a period. 2 reasons | Atomic radius DECREASES 1: Increasing nuclear charge due to an extra proton being added 2: There is no increase in screening effect as no new shell is being added |
| Electronegativity | A measure of an atom's ability to attract and hold electrons in a molecule. Will predict how atoms combine chemically. Linus Pauling developed the electronegativity scale. |
| Trends in Electronegativity going down a group. 2 reasons | Electronegativity DECREASES as we go down a group 1: Increasing atomic radius means the electrons are further away from the attractive force of the nucleus. 2: The screening effect of the inner negative electrons block the pull of the positive nucleus. |
| Trends in Electronegativity going left to right across a period. 2 reasons | Electronegativity INCREASES going across a period. 1: Increasing nuclear charge means the nucleus has a stronger hold on the electrons. 2: Decreasing atomic radius: as no new shell is being added the stronger nucleus can hold the outer electrons tighter |
| Ionization Energy | The first ionization energy of at atom is the minimum energy required to completely remove the most loosely bound electron from a neutral atom in a gaseous state. Noble Gases have the highest Ionization Energy levels, as they have full outer energy level |
| Trends in Ionization energy going down a group: 2 reasons | Ionization Energy DECREASES going down a group. 1: As atomic radius increases the electrons are further away from the nucleus. 2: The screening effect of the inner electrons cancels out the pull of the nucleus. |
| Trends in Ionization energy going left to right across a period: 2 reasons | Ionization Energy INCREASE going across a period 1: Increasing nuclear charge means the nucleus has a better hold on the outer electrons. 2: Decreasing atomic radius means that the outermost shell is closer to the nucleus and is therefore held tighter. |
| Reactivity of the Alkali Metals | Increases as we go down the group. All the elements have only 1 electron on their outer shell. Losing this electron gives them a full outer shell. This means they have a low ionisation energy and electronegativity. |
| Properties of Alkali Metals | 1: Easier to cut as we move down the group. 2: Display more vigorous reaction with water as we move down the group. 3: Tarnish with air faster as we move down the group. |
| Halogens | Have the highest Electron Affinity |
| Electron Affinity | The amount of energy required to add an electron to a neutral atom to form a negative ion or anion. How strongly an atom attracts additional electrons |
| Trends in Electron Affinity going left to right across a period | INCREASES from left to right along a period 1. as energy level continues to fill it has a stronger attraction for the electrons. |
Created by:
IcanDance
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