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across the period, elements change from metallic to non-metallic

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from the left to right, the properties of the oxides change from basic to amphoteric to acidic.

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Across the period from Na to Al, the elements are metal, then from Si to Ar, the elements are non metal.

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Elements go from metal to non-metal, exhibiting less metal-like properties as it goes from left to right.

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chemical properties will be different as all elements have different number of valence electrons, resulting in reactivity of elements to decrease along the period

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Physical prop properties are different. The number of neutrons, electrons and protons will increase. They have different physical properties because each element has a different atomic mass

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From left to right, the elements change from metallic to non-metallic

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different physical properties due to the different number of neutrons, resulting in lower electrical conductivity across the period

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the structure of the oxides of the elements from left to right are giant ionic crystal lattice structure to simple molecular structure.

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The chemical properties will be different.
A metallic element can react with acid to form hydrogen gas and a salt, but a non metallic element cannot. The chemical properties depend on the number of valance electrons in the element, so the chemical properties will be different

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From left to right, the elements change from metallic properties to non-metallic properties

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The chemical properties of the elements in period 3 differ across the period as the number of valence electrons is what determines the chemical properties. Since the elements across the periods are in different groups, they have different valence electrons and they have different chemical properties

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Sodium, Magnesium — Basic oxide
Aluminum — Amphoteric oxide
Silicon, Phosphorous, sulfur, chlorine — Acidic oxide
Argon — (does not react with oxygen)

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From Na to Al, ionic structures are formed.
From Si to Cl, covalent structures are formed.
No one cares about Argon.

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the physical properties of the elements will differ because they have different numbers of neutrons

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as we move from left to right of a period, atomic mass increases and electrons also increase, valence electrons are also different

reactivity decreases from left to right

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across the period, the compounds change from ionic to covalent. argon does not form an oxide

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From left to right, the oxides change from alkali/basic oxides to acidic oxides (except Argon, which is unreactive)
Eg.
NaO - Basic oxide
Al2O3 - Amphoteric oxides
SO2 - Acidic oxide

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Sodium, Magnesium — reacts with acid to form salt and water
Aluminum — reacts with acid and alkali to form salt and water
Silicon, Phosphorous, sulfur, chlorine — reacts with alkali to form salt and water
Argon — (does not react with oxygen)

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different physical properties exhibited due to different atomic masses, which causes varying degrees of electrical and heat conductivity, as well as solubility .

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from left to right, the oxides change from reacting with acids to form salt and water to reacting with bases to form salt and water (excluding argon, which is unreactive/inert)

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across the period, the oxides change from basic to acidic

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from left to right, the melting and boiling point is from high to low.
from left to right, the electrical conductivity is able to conduct electricity to unable to conduct electricity.
from left to right, the elements change move from being soluble in water but insoluble in organic solvents, to being insoluble in water but soluble in organic solvents

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Na and Mg form basic oxides, reacting with acids
Al forms an amphoteric oxide, reacting with both acids and alkalis
Si to Cl form acidic oxides, reacting with alkalis

Argon has no one.

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oxides of sodium and magnesium react with acids, aluminium oxides reacts with both acids and bases, the rest of the oxides reacts with bases except for argon

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for the metal oxides,
a giant ionic crystal lattice structure is formed
For the non-metal oxides, a simple molecular structure is formed.
Argon does not react with oxygen

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The structure of the oxides of sodium, magnesium and aluminium is giant ionic crystal lattice structure. Silicon dioxide forms a macromolecular structure. The oxides of phosphorus, sulfur and chlorine forms simple molecular structure. Argon is in group 0 and hence, unreactive.

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From Na to Al, the elements exhibit metallic properties

From Si to Ar, the elements exhibit non-metallic properties

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for elements on the left, giant ionic crystal lattice structure are formed, for elements in the centre, macro molecular structures are formed , for elements at the right, simple molecular structures are formed and for elements in group 0, no reaction with oxygen and hone no oxides formed.

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From left to right, the oxides formed with the elements change from giant ionic crystal lattice structures to macro molecular (SiO) and simple molecular structures

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Different, because no. of valence electrons that are involved in boning increases down the period

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The number of valence electrons increases from left to right. As the number of valence electrons determine the chemical properties of an element, as it determines how it bonds with another element, the chemical properties differ from each element.

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oxides of Na and Mg are basic, oxide of aluminium is amphoteric and oxides of sulcus are acidic in nature

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From left to right, the elements’ physical appearances change from shiny to dull, and their melting and boiling points also decrease from left to right.

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from left to right, oxides formed react with acids, with both acids and bases, and to bases. In group 0, no reaction would be present.

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Basic oxides (Na, Mg)
- Oxides of metals
- Solid at room temperature
- Reacts with acids to form salt and water only

Acidic oxides (Si, P, S, Cl)
- Oxides of non-metals
- Gases or volatile liquids at room temperature
- Reacts with alkalis to produce salt and water only

Amphoteric oxides (Al)
- Oxides of metals
- Can react with both acids and alkalis to produce salt and water only
- Eg. Zinc oxide, Aluminium oxide, Lead(ll) oxide

Neutral oxides (Ag)
- Do not exhibit acidic nor alkaline properties
- Eg. CO, NO, H2O

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From left to right, the elements change from alkali to acidic properties

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The number of neutrons increase from left to right, affecting the atomic masses of each element. This in turn affects the physical properties of the elements, affecting their electrical and heat conductivity, their solubility and density.

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Down the period, melting point and boiling point gets lower. Na, Mg and Al can conduct electricity.