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From left to right across a period, the elements become less metallic

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metallic elements form cations and non-metallic elements form anions as metallic elements are generally located in groups 1-3 with less valence electrons and hence lose them more readily

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From left to right, metallic properties of metals decrease and non-metallic properties of metals increase.

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chemical properties of the elements are different because the number of valence electrons differ across the period

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from left to right the elements get less metallic , from sodium to aluminium it is metal and from silicon to argon it is non-metallic

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Different chemical properties, diff number of valence electrons

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Chemical properties are different

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Physical properties are different

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chemical properties are different as number of valence electrons differ, and number of valence electrons determine an elements chemical properties

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- sodium magnesium and aluminium are metallic (more metallic)
- silicon phosphorus sulfur and chlorine are non-metallic (non metallic)

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Different physical properties, different atomic mass

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elements sodium, magnesium and aluminium exhibit metallic properties whereas elements silicon, phosphorus, sulfur, chlorine and argon exhibit non metallic properties

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Different physical properties due to different relative atomic mass

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they have different physical properties as the atomic masses are different

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- they have different chemical properties as they have varying Valence electrons

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The first three elements are metallic, the last five elements are non-metallic. The metallic properties correspond with group numbers, the smaller ones (Grp 1-3) being metallic and the larger ones (group 4 onwards)being non-metallic.

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Chemical properties are different because:
1) they have different number of valence electrons
2) some are metals, some are not, so reactions are categorised differently. Between the metals, reactions can also differ eg. by speed

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Metals form giant ionic crystal lattice structure but non metals forms simple molecular and giant molecular structure

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different because they have different number of valence electrons

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Metallic substances are substances which loses its valence electrons easily to get a positive cation with a stable noble gas configuration and a sea of delocalised electrons. This happens more from the earlier group numbers

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- they have different physical properties as the number of neutrons is increasing across the period

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different as there are different number of valence electrons ; sodium , aluminium , magnesium can conduct electricity , high melting and boiling point , insoluble in water ; silicon , phosphorous , sulfur , chlorine , argon cannot conduct electricity

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The thermal stability of the oxides of the elements decreases from the left to the right of the period, as the atomic mass increases

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Physical properties are different due to different number of neutrons and protons in each atom
Each atom have different atomic mass

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Metals can conduct electricity in solid and molten state. Non metals cannot conduct electricity at all except graphite.

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metals will form a giant metallic crystal lattice structure and non-metals will form a simple molecular structure

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Stable
Metals react to form acidic oxides, non-metals react to form basic oxides

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The metallic atoms would be oxides with ionic bonds between the positively charged cations and the negatively charged anions to have a giant ionic crystal lattice structure. The non-metallic atoms would form oxides that had a simple molecular structure with strong covalent bonds.

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the metallic elements from the left side of the period form oxides with a giant ionic crystal lattice structure while the non-metallic elements on the right side of the period form oxides with a simple molecular structure

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Metallic oxides react with acids to form salt and water, Non-metallic oxides react with alkali to form salt and water

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They react more with bases as the groups increase

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Metal oxides are basic, non metal oxides are acidic

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the oxides are basic to acidic. sodium and magnesium form basic oxides. aluminium forms amphoteric oxide and non metals like sulfur will form acidic oxides

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The have the same number of valence shells of 3.

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Elements on the right are metals an form giant metallic crystal lattice structures, elements on the left are non metals and form simple/ giant molecular structures

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- sodium and magnesium’s oxides form basic oxides while aluminium oxide forms amphoteric oxide
- the non-metals in period three form acidic oxides

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Metals form cations to react with oxides to form an ionic crystal lattice structure. Non-metals share electrons to bond with oxygen, forming a simple molecular structure. This corresponds with the metallic properties of atoms, in the sense that the first three elements are the ones to form ions and the last four are to form molecules.

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The first 2 elements of period 3 form basic oxides, aluminium forms amphoteric oxide, elements in group IV to VII form acidic oxides while Argon is unreactive.

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The metals form ionic bonds with oxygen while non-metals form covalent bonds oxygen

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From left to right, the oxides of the elements behaves as a basic oxide which reacts with acids, to an amphoteric oxide which reacts with both acids and alkalis and to acidic oxides which reacts with alkalis

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Metals will form oxides with giant ionic crystal lattice structure, whereas non-metals produce oxides with simple molecular structure.

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elements like sodium and magnesium oxide will form a giant ionic crystal lattice while non metals such as sulfur will form a simple molecular structure, sulfur dioxide

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They have different chemical properties a they have a different number of valence electrons so the different atoms would react differently.

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metal oxides conduct electricity in aqueous and molten state while non metal oxides do not conduct electricity in any state except for graphite

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Metal oxide can conduct electricity in molten and aqueous state, non-metal oxide cannot conduct electricity because it exist as molecules
Metal oxide have high melting and boiling point, non metal oxide have Low melting and boiling point
Argon do not form oxides because it is unreactive
Silicon dioxide have high melting and boiling point

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As the period moves from left to right the elements get less reactive and hence it’s compound will get less stable to heat and will get displaced more easily

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The metals in period 3 form basic oxides that reacts with acids to form salt and water
Aluminium oxide form amphoteric oxide which reacts with both acids and alkalis
The non metals form acidic oxides that reacts with bases to form salt and water

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the basic oxides are able to react with acids to form salt and water
the amphoteric oxides react with both acids and alkalis to form salt and water
the acidic oxides react with alkali to form salt and water
sodium magnesium and aluminium (metals) are decreasing in reactivity -> decreasing thermal stability

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As the oxides of the elements move from left to right, the thermal stability decreases
Argon does not form oxides as it is a noble gas