Chemistry, 30.08.2019 22:40 mrashrafkotkaat

The elements in group 2 are classified as(1) metals (3) nonmetals
(2) metalloids (4) noble gases

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Answer from: kiki4832

The correct answer is Option 1.

Explanation:

From the given options:

Option 1: Metals

Metals are defined as the elements which loose its electrons in order to attain stability. Most of the periodic table consist of metals. Elements belonging to Group 1 to 13 are considered as metals.

Option 2: Non-metals

Non- metals are defined as the elements which gain electrons in order to attain stability. Elements belonging to Group 14 to 17 are considered as non-metals.

Option 3: Metalloids

Metalloids are defined as the elements which show the property of both metals and non-metals. There are 7 metalloids in the periodic table. they are Born (B), Silicon (Si), Germanium (Ge), Arsenic (As), Antimony (Sb), Tellurium (Te) and Polonium (Po).

Option 4: Noble gases

The elements which belong to Group 18 are considered as noble gases. They are Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe) and Radon (Rn).

Hence, elements in Group 2 will be classified as Metals.

Thus, the correct answer is Option 1.

Answer from: Quest

assuming that your periodic table has eighteen columns, you should highlight the four elements in the third column from the left of the table.

explanation

neutral atoms of elements after calcium contain d electrons. the energy of d orbitals of a particular main shell lies between the energy of the s and p orbitals of the next main shell. for example, electrons in the $3d$ have energy higher than those in the $4 s$ orbital while lower than those of the $4 p$ orbital.

by the aufbau principle, electrons fill orbitals one at a time, starting from those of the lowest energy. the $4s$ orbital is therefore filled right after $3p$ orbitals and before $3 d$ orbitals.

potassium has electron configuration $[\text{ar}] 4 s^{1}$ and calcium $[\text{ar}] 4 s^{2}$ . the s orbital of a main shell holds a maximum of two electrons. the next element would thus have the electron configuration $[\text{ar}] 4 s^{2} \; 3d^{1}$ and satisfy the requirements.

a neutral atom of the element contains three electrons on top of the most recent noble gas element. it should thus be placed in the third column of the periodic table. both scandium and yttrium would satisfy the conditions. an aufbau diagram indicates that the 4f orbital is filled before the 5d. however, it appears that exceptions exists for both lanthanum and actinium. neutral atoms of the two d-block elements also demonstrate the $ns^{2} \; (n-1) p^{1}$ and should be highlighted as well.

Answer from: Quest

Iwould you figure it out but you don't have a picture or in your question as to what the physical property you're looking for is

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The elements in group 2 are classified as(1) metals (3) nonmetals
(2) metalloids (4) noble gas...