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Chapter 4: Problem 15

Column A \(\quad\) Column \(\mathbf{B}\) A. s-block () a. Radioactive metal B. Fluorine () b. Highest first IP value C. Chlorine () c. Lanthanides D. d-block () d. Highly reactive metals E. 4 f-series () e. Heavy metals E Helium () f. Always form \(-1\) oxidation state G. Francium ( ) g. Highest electron affinity value H. Noble gases () \(\mathrm{h}\). Zero group elements

Short Answer

Expert verified
Question: Match the elements or properties in Column A with their descriptions in Column B. Column A: 1. s-block 2. Fluorine 3. Chlorine 4. d-block 5. 4 f-series 6. Helium 7. Francium 8. Noble gases Column B: a. Radioactive metal b. Highest first IP value c. Lanthanides d. Highly reactive metals e. Heavy metals f. Always form -1 oxidation state g. Highest electron affinity value h. Zero group elements Answer: 1. d 2. f 3. g 4. e 5. c 6. h 7. a 8. b

Step by step solution

01

Identify the properties of each element or group in Column A

A. s-block: Elements have their outermost electron in an s-orbital, includes alkali metals and alkaline earth metals. B. Fluorine: A highly reactive nonmetal, having the highest electronegativity and ionization energy in its period. C. Chlorine: A highly reactive nonmetal and a halogen. D. d-block: Consists of transition metals. E. 4 f-series: Consists of the lanthanides. E Helium: Lightest noble gas with a full outer shell. G. Francium: Alkali metal with the lowest electronegativity. H. Noble gases: Elements with a full outer shell and very low reactivity.
02

Match the elements or properties in Column A with their descriptions in Column B

A. s-block matches () d. Highly reactive metals: s-block contains alkali and alkaline earth metals which are highly reactive. B. Fluorine matches () f. Always form \(-1\) oxidation state: Fluorine, a halogen, forms a \(-1\) oxidation state due to its high electronegativity. C. Chlorine matches ( ) g. Highest electron affinity value: Chlorine is a halogen and has one of the highest electron affinity values among nonmetals. D. d-block matches () e. Heavy metals: d-block consists of transition metals which are commonly referred to as heavy metals. E. 4 f-series matches () c. Lanthanides: The elements in the 4 f-series are called lanthanides. E Helium matches () \(\mathrm{h}\). Zero group elements: Helium is a noble gas and belongs to the zero group elements as they have an oxidation state of zero. G. Francium matches () a. Radioactive metal: Francium is an alkali metal and is radioactive due to its unstable atomic nucleus. H. Noble gases match () b. Highest first IP value: Noble gases have a full outer electron shell, resulting in the highest first ionization potential value in their respective periods.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding s-block Elements
The s-block elements on the periodic table include the highly reactive family of alkali metals and the slightly less reactive alkaline earth metals. This group gets its name because the electrons added to these elements fill their s-orbital.

Alkali metals, found in Group 1 of the periodic table, have a single valence electron, which they readily lose to form positive ions with an oxidation state of +1. They are known to react vigorously with water and halogens. As we move down the group from lithium to francium, the reactivity increases.

Alkaline earth metals, located in Group 2, have two valence electrons leading to a common oxidation state of +2. They're also reactive, though less so than their Group 1 counterparts.

These s-block metals are characterized by their soft texture, shiny appearance, and good conductivity of electricity and heat. They have wide applications in industries, from electronics to pharmaceuticals.
Halogens Reactivity
Halogens, found in Group 17 of the periodic table, are comprised of fluorine, chlorine, bromine, iodine, and astatine. These nonmetals are particularly reactive due to their seven valence electrons; they are eager to gain an extra electron to achieve a stable octet configuration.

Fluorine, the most electronegative element, tops the list with its ability to form a -1 oxidation state and has the highest electron affinity, which explains its extreme reactivity. Its compounds, particularly with alkali metals, are often used in toothpaste and water treatment.

Moving down the group, reactivity decreases, but these halogens still form salts when reacting with metals and create various organic and inorganic compounds essential in manufacturing, medicine, and more.
d-block Transition Metals Characteristics
Transition metals are found in the d-block of the periodic table and are characterized by their d-orbitals being filled with electrons. They typically display multiple oxidation states, high melting points, and the ability to form colored compounds.

Metallic Properties and Magnetism

These metals, including iron, copper, and nickel, are known for their strength and metallic luster. Many of them exhibit magnetic properties, with iron being the most familiar example.

Catalytic Activity

Moreover, transition metals are notable for their catalytic activity, playing a crucial role in industrial processes like the Haber-Bosch method for producing ammonia.

Alloys and Coordination Compounds

They also form various alloys and complex coordination compounds. Jewelry, coins, and electronics often utilize the desirable properties of d-block metals.
Lanthanides 4 f-series Exploration
The lanthanides, which constitute the f-block of the periodic table, are a series of 15 elements from lanthanum through lutetium. These elements have electrons that primarily occupy the 4f sublevel.

Hard to Separate

Chemically similar, these metals are hard to separate and are often found together in nature. They have high melting points and are typically silvery in appearance. Despite being termed as 'rare-earth elements,' they are relatively abundant in the Earth's crust.

Applications in Technology

Lanthanides are used in various high-tech applications, from smartphone screens and electric vehicle batteries to medical MRI contrast agents. Their unique magnetic, phosphorescent, and catalytic properties have made them integral to modern technology.

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Most popular questions from this chapter

The formulae of oxides formed when barium burns in presence of oxygen are (a) \(\mathrm{Ba}_{2} \mathrm{O}, \mathrm{BaO}\) (b) \(\mathrm{BaO}, \mathrm{BaO}_{2}\) (c) \(\mathrm{BaO}, \mathrm{Ba}_{2} \mathrm{O}_{2}\) (d) \(\mathrm{B}_{2} \mathrm{O}, \mathrm{B} a \mathrm{O}_{2}\)

An element with atomic number " 32 " belongs to (a) 4 th period, VIA group (b) 3 rd period, IVA group (c) 4 th period, IVA group (d) 5 th period, VA group

Which of the following sequence of explanation is appropriate for explaining the reason for the periodicity of reducing property in a period or group? (1) Tendency to undergo oxidation decreases in a period and increases in a group. (2) In a period ionization energy increases and in a group it decreases. (3) In a period the atomic size decreases and in a group it increases. (4) The elements present in the left side of the periodic table have strong reducing property. (a) 3214 (b) 3421 (c) 4312 (d) 4213

The element having the electronic configuration \([\mathrm{Kr}] 4 \mathrm{~d}^{10} 4 \mathrm{f}^{14} 5 \mathrm{~s}^{2} 5 \mathrm{p}^{6} 5 \mathrm{~d}^{2} 6 \mathrm{~s}^{2}\) belongs to (a) s-block (b) p-block (c) d-block (d) f-block

State whether the following statements are true or false. The inert gas present in the second long period is Xe.
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