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Test: Classification of Elements and Periodicity in Properties - Chemistry MCQ


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15 Questions MCQ Test - Test: Classification of Elements and Periodicity in Properties

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Test: Classification of Elements and Periodicity in Properties - Question 1

Examining periodic trends in the ________ is done using the periodic classification of elements.

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 1

The electronic arrangement of atoms, which is used to study the physical and chemical properties of the elements, has a logical effect on the periodic classification of elements.

Test: Classification of Elements and Periodicity in Properties - Question 2

An element's electrical configuration is 1s2, 2s2, 2p6, 3s23p3. What is the atomic number of the element in the periodic table that is immediately below the one above?

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 2

The sum of all the electrons in the given electronic configuration will determine the atomic number. The element that is present just below the given element will have an outermost electronic configuration as 4s24p3, hence, its full electronic configuration will be 1s2,2s22p6,3s23p6,4s2, 3d10,4p2. Thus, its atomic number is 33.

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Test: Classification of Elements and Periodicity in Properties - Question 3

What electronic arrangement of an atom has the lowest ionization enthalpy among the following?

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 3

The amount of energy needed to remove one electron from an isolated gaseous atom's outermost orbit is known as the ionization enthalpy. The ionization enthalpy is lowest for the electronic structure 1s22s22p63s1.

Test: Classification of Elements and Periodicity in Properties - Question 4

 An element with the atomic number 15 has the following group number, valence electron count, and valency values, in that order:

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 4

Atomic number 15 (Z) belongs to P, this can be written as [Ne] 3s23p3
Phosphorus is in group 15 of elements. In the ground state, the valence electron count for phosphorus is 5 and the valency is 3, from 3s23p3.

Test: Classification of Elements and Periodicity in Properties - Question 5

The cation's ionic radius is always _____.

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 5

The cation's ionic radius is always less than its atomic radius. The loss of electrons produces cations. Ionic radius decreases as a result of the rise in effective nuclear charge.

Test: Classification of Elements and Periodicity in Properties - Question 6

Sort S, O, and Se according to their increasing electron affinities

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 6

A group's electron affinity declines as its atomic number rises. Se, O, and S are all group 16 elements. Thus, the expected order of their increasing electron affinities would be O > S > Se. However, this is not the observed case as the oxygen atom is extremely small. So, oxygen cannot hold a negative charge in such a small space. Therefore, the electron affinity of oxygen is the lowest in the group. 

Test: Classification of Elements and Periodicity in Properties - Question 7

Which of the following oxides has the characteristics of an amphoteric?

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 7

SiO2 is slightly acidic, CaO is basic, and CO2 is acidic. SnO2 is amorphous.

Test: Classification of Elements and Periodicity in Properties - Question 8

The element next to F on Pauling's electronegativity scale is

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 8

The ability of an atom in a molecule to draw electrons toward it is known as electronegativity, according to Pauling. When we examine the periodic table's trend, we can observe that while electronegativity increases between periods, it drops as we move down the groups. Pauling estimated the differences in electronegativity between the atoms in a covalent bond based on the bond energies and assigned the most electronegative element, fluorine, a value of 4, and other elements were calculated concerning that value. So, on Pauling's scale, oxygen is the element following fluorine.

Test: Classification of Elements and Periodicity in Properties - Question 9

The ionization enthalpies of the elements decline from top to bottom in a group of the periodic table due to ________.

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 9

The atomic size increases down the periodic table. Due to a rise in atomic size, a set of elements in the periodic table have ionization enthalpies that drop from top to bottom.

Test: Classification of Elements and Periodicity in Properties - Question 10

Despite being in separate groups, lithium and magnesium have remarkably similar chemical makeup. It does so for several reasons, including the following:

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 10

Their charge density, or the ratio of charge to size, is very similar. Even though they are grouped differently due to a diagonal relationship, lithium and magnesium have remarkably comparable chemical properties.

Test: Classification of Elements and Periodicity in Properties - Question 11

The atomic radii of the elements O, S, Se, and As are rising in size in the following order:

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 11

Atomic radii increase as you move down in a group as new shells are added one at a time, which is why O < S < Se. Additionally, As is in group 15 and has one fewer electron in its p orbital than group 16 elements, giving it a bigger atomic radius. Thus, O < S < Se < As.

Test: Classification of Elements and Periodicity in Properties - Question 12

The period in the current periodic table denotes the value of the following quantities:

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 12

The chemical elements are arranged in a periodic table according to their atomic number (the number of protons in the nucleus), electron configurations, and characteristic chemical properties. A period in the Modern Periodic Table is indicated by the value of the primary quantum number (n) for the outermost shell or the valence shell.

Test: Classification of Elements and Periodicity in Properties - Question 13

Elements of which of the following parts exhibit the property of decreasing atomic size with increasing atomic number.

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 13

A trait of elements in the f-block is the decrease in atomic size with the increase in atomic number. Both lanthanoid and actinoid contractions refer to it. This is brought on by the f subshell's electrons' inadequate shielding.

Test: Classification of Elements and Periodicity in Properties - Question 14

Which order best depicts the oxides' progressively less acidic nature?

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 14

The typical oxides of elements become more acidic as you move from left to right in a period as their electronegativity rises.

Test: Classification of Elements and Periodicity in Properties - Question 15

Elements that are considered to be representative elements are those that belong to

Detailed Solution for Test: Classification of Elements and Periodicity in Properties - Question 15

The term "representative elements" refers to substances with complete inner shells but incomplete outer shells, i.e., substances with fewer than 8 electrons in the outermost shell. Except for inert gas, the s and p block elements are referred to as representative elements.

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