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Structure of oxide refers to bonding structures - ionic giant crystal lattice structure, giant covalent structure, simple covalent structure.

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Sodium, Magnesium, Aluminium are metals. They can conduct electricity.

Silicon, Phosphorus, Sulfur, chlorine, argon are non metals

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The metal elements are grouped in group 1,2,13, and the non metals follow from group 14-18. Transition metals are from group 3-12.

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From sodium to aluminium, the elements are metallic. From silicon to argon, the elements are non-metallic

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Higher Bp and MP —> Lower BP and MP
More reactive —> less reactive
Number of valence electrons increases

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Sodium, magnesium and aluminium are metals: therefore exhibit the properties of metals

Silicon, phosphorus, sulfur, chlorine and argon are non-metals: therefore exhibit the properties of non-metals

Identified by the line that separates metals and non-metals in the periodic table as well as the number of valence electrons, identified by the group number of the elements

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From Group 1-3, the elements are metallic and can conduct electricity. From Group 4-8, the elements are non-metallic and thus cannot conduct electricity.

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The chemical properties change as it goes across Period 3 as the number of valence electrons giving the elements the chemical properties increases.

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They will be different as they are not in the same group.

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They are different because they are not in the same group

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It will be different due to the different number of neutrons from left to right of the periodic table.

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The elements from sodium to aluminium bond with oxygen to form a ionic oxide while the elements from silicon to chlorine bond with oxygen to form a covalent oxide and argon is a noble gas and does not react with oxygen

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Different. Different number of valence electrons. Number of valence electrons increases across the period.

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The physical properties change across the Period as the number of neutrons increases.

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The physical properties of the elements are different as they are in different groups

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Metal oxides are basic in nature and exists as solids at room temp. They react with acids to form salt and water. Non metal oxides are acidic in nature and exists mostly as gas at room temperature. They dissolve i’m water to form acids

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The elements are in different groups and hence possess different chemical properties, such as their valency

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The metal and non-metal elements all have different physical properties, like how the elements bond differently to each other, leading to different melting and boiling points, and solubility.

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The chemical properties are different as the valence electrons determines the chemical properties. Across the period, the elements have an increase in the valence elections, thus their chemical properties will be different.

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Don't forget the aluminium oxide which is amphoteric

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The metals will form ionic bonds with oxygen and non-metals form covalent bonds with oxygen. Argon will not form an oxide as it is a noble gas

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Sodium to Aluminium bond with oxygen to form basic oxides. Silicon to chlorine bond with oxygen to form acidic oxides. Argon is a noble gas that does not react with anything.

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metal forms ionic bonds
non metals can form ionic, covalent etc. bonds

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Aluminium bonds with oxygen to form an amphoteric oxide

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Basic oxides like sodium oxide, magnesium oxide react with acid to form salt and water and is solid in room temperature. Amphoteric oxides like aluminium oxide reacts with a both acid and alkali to form salt and water. Acidic oxides like silicone oxide, phosphorus oxides, sulfur oxide, etc reacts with alkali to form salt and water while argon is a noble gas and is non metallic and doesn’t form oxides

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The metals form ionic bonds with oxygen and the non-metals form covalent bonds. Argon is a noble gas and does not bond with oxygen

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The metallic elements form basic oxides.
Aluminium forms an amphoteric oxide. Non-metallic elements
form acidic oxides.

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Na, Mg form basic oxides as they are metals.

Al forms amphoteric oxides.

Si, P, S and Cl form acidic oxides as they are non metals.

Ar does not form an oxide as it is unreactive.

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Physical properties are likely to differ-
Na to Al:
1. Shiny
2. Malleable and ductile
3. high mp and bp
4. good conductor of electricity
5. Good conductors of heat

Si-Ar:
1. Dull
2. Brittle
3. low mp and bp
4. bad conductor of electricity
5. poor conductors of heat

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Metals bond to form basic oxides, whereas the non metals such as silicon oxide are acidic.

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Sodium and magnesium form basic oxides. Aluminium forms an amphoteric oxide. Silicon to chlorine form acidic oxides.

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acidic oxides formed by non metals have low pH while basic oxides formed by metals have higher pH

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They have different chemical properties as they have the same number of electron shells (same period) but different number of valence electrons (different groups). They have different physical properties as some elements are metal while others are non-metal elements.

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The metallic elements- sodium and magnesium are basic oxides. However, aluminium is an amphoteric oxide. The non-metallic elements are acidic oxides.

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metals and non-metals have different physical properties
for eg. certain metals combine with oxygen to form oxides

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Acidic oxides react with water to form acids.
Basic Oxides react with water to form alkalis
Amphoteric Oxides react with both acid and alkali to form salt and water.

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The metallic elements form ionic bonds with oxygen. Non-metallic elements form covalent bonds with oxygen.

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Sodium to aluminium(metals)conduct electricity while silicon to chlorine(non-metals) do not conduct electricity.

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Acidic oxides form acids when dissolved in water and react with alkalis to form salt and water only. Basic oxides form alkalis when dissolved in water and react with acids to form salt and water only. Amphoteric oxides can react with both acids and alkalis to form salt and water only.