the atomic radius decreases across period 3 because the force of attraction between the nucleus and...
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![Page 1: The atomic radius decreases across Period 3 because the force of attraction between the nucleus and the electrons increases](https://reader036.vdocument.in/reader036/viewer/2022070401/56649f1d5503460f94c34053/html5/thumbnails/1.jpg)
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The atomic radius decreases across Period 3 because the force of attraction between the nucleus and the electrons increases.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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There are more electrons, but a negligible increase in shielding because each extra electron enters the same shell.
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The first ionisation enthalpy increases across Period 3. The force of attraction between the nucleus and the outer electron increases.
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The first ionisation enthalpy increases across Period 3. The force of attraction between the nucleus and the outer electron increases.
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The first ionisation enthalpy increases across Period 3. The force of attraction between the nucleus and the outer electron increases.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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The number of protons in the nucleus and the nuclear charge increase.
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There are more electrons, but little increase in shielding as each extra electron enters the same shell.
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The density of an element is its mass per unit volume. It is a measure of how closely its particles are packed.
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The density of the metals increases across the period.
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Silicon has a densely packed giant covalent structure.
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Phosphorus and sulphur exist as the simple molecules P4 and S8, and are less dense.
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Chlorine and argon are both gases at room temperature, so their densities are very low.
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When a substance melts or boils, attractive forces holding the particles together must be overcome.
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The stronger the attractive forces are, the more energy is needed to overcome them.
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Sodium, magnesium and aluminium are all metals. They have strong metallic bonding.
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Silicon has a giant covalent structure in which its atoms are joined by strong covalent bonds.
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There are weak instantaneous dipole–induced dipole attractions between phosphorus, sulphur and chlorine molecules.
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There are weak instantaneous dipole–induced dipole attractions between argon atoms. Little energy is needed to overcome them.
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Sodium, magnesium and aluminium are metals with delocalised electrons that can move and carry charge.
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Sodium, magnesium and aluminium are metals with delocalised electrons that can move and carry charge.
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Sodium, magnesium and aluminium are metals with delocalised electrons that can move and carry charge.
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Each aluminium atom contributes more delocalised electrons than sodium or magnesium.
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Silicon is a semiconductor. It is used in computer circuitry.
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Phosphorus, sulphur and chlorine are simple molecules with no free electrons.Argon exists as single atoms.