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They go basic to neutral to acidic

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They are progressively less reactive
Their proton number increases

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Elements till group 13 are metals while the elements in group 14-18 are non metals

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From left to right the elements progressively decrease in its metallic properties.

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Period 3 elements become less metallic as we move from left to right.

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- Their metallic properties decrease from left to right
- Elements from group 1-13 are metals and elements in group 14 onwards are non-metals

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Elements in period 3 are metallic up till group 13. Elements after are non-metallic.

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Elements in period 3 have different chemical properties as we move from left to right. This is because the elements have increasing number of valence electrons when we move from the left to right.

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From left to right, the electrical conductivity of the elements decrease

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Elements in Period 3 have different chemical properties as they have different charges and valence electrons.

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Different
The metals in period 3 lose their valence electrons to form positive ions while the non- metals will gain electrons to form negative ions.

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It gets less reactive from left to right
They have a more valance shells as they move from left to right

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Elements in period 3  have different physical properties as the atomic number increases from left to right.

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The elements in period 13 have an increasing atomic mass as you move from left to right.

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Different. Since chemical properties depend on the number of valence electrons and elements in the period have different number of valence electrons, they have different chemical properties

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- The metals from group 1-13 lose their valence electrons while the non-metals from group 14 onwards gain electrons.

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The metals will combine with oxygen to form ionic bonds while the non metals will combine with oxygen to form simple covalent bonds.

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The number of valance electrons increases from group 1 to 18

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Elements have similar physical properties because of its increasing atomic mass.

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The structure of the oxides of period 3 elements go from an ionic crystal lattice structure to simple molecular as we move from left to right- not including Argon, which is unreactive.

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Period 3 elements have different chemical properties. This is possibly due to two reasons. (1) Some elements are metallic while others are not metallic. (2) Elements have different number of valence electrons

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- They have different physical properties - the metals are good conductors of heat while the non-metals are poor conductors of heat
- The metals have high melting and boiling points while the non-metals have low melting and boiling points

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Sodium oxide is basic, Magnesium oxide is basic, aluminium oxide is amphoteric, sulfur and silicon dioxide are acidic

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Different. The atomic radius decreases as you go along the period and they have the same valence shell hence their physical properties are different.

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Basic oxides 🐂 - sodium and magnesium
Amphoteric - aluminium
Acidic -sulfur and silicon dioxide

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The pH of the oxides of period 3 elements decrease as we move from the left to right- not including Argon, which is a noble gas and is thus unreactive.

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They react with either acids or bases to from salt and water.

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The nature of oxides changes from basic to amphoteric to acidic as the pH level decreases as we progress through period 3.

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These oxides react with acids to form salt and water.

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The metallic elements in period 3 will form ionic bonds to form a giant ionic crystal lattice structure, while the non-metallic elements will form covalent bonds to form a simple molecular structure.

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The basic oxides react with acids while the acidic oxides react with alkali to form salt and water. The amphoteric oxides can react with both acids and alkali.

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- the non-metals combine with other non-metals to form covalent bonds -> Simple molecular structure (Argon does not react)

- the metals combine with non-metals to form ionic bonds -> giant ionic crystal lattice structure

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They are able to react with different chemicals (acidic and alkaline) to form substances

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Metallic elements (for example magnesium) form basic oxides that react with acid to form water and salt, and also turns moist red litmus paper blue.
Aluminium forms amphoteric oxides that react with both acid and alkali to form salt and water.
Non-metallic elements (for example sulfur) form acidic oxides that react with alkali to form water and salt, and also turns moist blue litmus paper red

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Giant crystal lattice structure to Simple covalent structure

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- They go from basic to amphoteric to acidic. Argon is a noble gas- does not react

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Basic oxides react with acids to form salt and water
Amphoteric oxides react with both acids and alkalis to form salt and water
Acidic oxides react with bases/alkalis to form salt and water