Question

PLEASE ANSWER...........WILL MARK BRAINLIEST!!!!!!!

Answer 1

The result of introducing a solution of alkali metal cations to a solution of halogen anions will form halide compounds which is soluble compound

Further explanation

The noble gas element is a stable of elements. The noble gas element is monatomic. Stability of noble gases is caused by an electron configuration that has a stable configuration of 8 (has 8 valence electrons) except He with a duplet configuration (has 2 valence electrons)

Other elements that do not yet have electron configurations such as noble gases will try to achieve their stability by forming bonds between elements.

This is generally called the octet rule

Group 1A elements from top to bottom, the easier the elements release electrons, and the more reactive

For this reason, IA elements (also called alkali metal elements) are highly reactive metals.

Alkaline element in the positive ion state (cation) is 1 (+)

The halogen elements have a high electronegativity so that it is easy to attract electrons to fill the electrons so that they are like noble gases

The halogen element in the negative ion state (anion) is 1 (-)

In modern periodic systems, the metal element is generally located on the left while the non-metal is on the right.

The formation of electron configurations such as noble gases can be done by sharing electrons with covalent bonds or hand over electrons with ionic bonds.

Alkali metal reacts with the halogen element to form halide compounds. General equation

2L (s) + X₂ (g) -> 2LX (s)

Examples of the reaction of Sodium alkali metals with halogens:

2Na (s) + Cl₂ (g) -> 2NaCl (s) (Sodium chloride)

For the solution, for example, the neutralization reaction of NaOH containing alkali Na⁺ and HCl which has the element Halogen Cl⁻

NaOH + HCl ---> NaCl + H2O

Bonding that occurs due to electron handover. Can occur in metal and non-metal atoms.

Like the alkali metal Na will release electrons to form Na + so that the electron configuration is stable as the noble gas element Ne

electron configuration Ne: [He] 2s2 2p6

Na electron configuration: [Ne] 3s¹

electron configuration Na + = [Ne] = [He] 2s2 2p6

While non-metallic Halogen elements like Cl will attract 1 electron so that the electron configuration is like Ar

electron configuration Ar: [Ne] 3s² 3p⁶

electron configuration Cl: [Ne] 3s² 3p⁵

electron configuration Cl- = [Ar] = [Ne] 3s² 3p⁶

The bond between alkali and halogen will form ionic bonding

Learn more

the octet rule

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calcium obey the octet rule when reacting to form compounds

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an exception to the octet rule

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Answer 2

Explanation:

Alkali metal cations reacts vigorously with halogens to form ionic/electrovalent compounds.

• The alkali metals are about the most reactive metals and they belong to group I .
• In their outermost shell, they have one valence shell electron.
• Alkali metals are largely electropositive willing to release their valence electron to attain stability.
• The halogens have seven electrons in their outermost shell. To complete their configuration, they need just one electron.
• All the halogens are strongly electronegative and they are readily reactive.
• In the vicinity of group 1 elements, they react vigorously.
• This is due to the electrostatic attraction between the metal and non-metal ion formed.
• Therefore, they form strong ionic bonds between their compounds.

Learn more:

sodium alkali and halogens brainly.com/question/6324347

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