Trends and Patterns in the Periodic Table
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| 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.
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| 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.
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| 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
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| 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.
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| 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.
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| 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
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| 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
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| 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.
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| 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.
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| 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.
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| 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.
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| Reactivity of the Halogens | Reactivity increases moving up the group.
1: Decreasing atomic radius brings the outer shell closer to the nucleus.
2: Electronegativity increases as we move up the group.
3: All the halogens require only 1 electron to achieve noble gas structure
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| 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
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| 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 elecrons.
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