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Chapter 4: Problem 2

State whether the following statements are true or false. In a period, the first element has the smallest size.

Short Answer

Expert verified
Answer: False. The atomic size decreases across a period from left to right due to an increase in the effective nuclear charge, making the last element in the period have the smallest size.

Step by step solution

01

Understand the structure of the periodic table

The periodic table is organized into rows called periods and columns called groups. Elements within a period have increasing atomic numbers, which affect their size and other properties.
02

Analyze the trend of atomic size in a period

As we move from left to right across a period, the number of protons in the nucleus increases, which causes an increase in the positive charge. This leads to a stronger attraction between the positively charged nucleus and the negatively charged electrons. At the same time, electrons are added to the same energy level (the same principal quantum number), so the shielding effect remains constant. This means that the effective nuclear charge (which is the net positive charge experienced by an electron) increases across a period, making the electron cloud more tightly held by the nucleus.
03

Determine whether the statement is true or false

Based on the analysis in Step 2, we can conclude that atomic size decreases across a period from left to right due to an increase in the effective nuclear charge. Therefore, the statement "In a period, the first element has the smallest size" is False. The atomic size decreases across a period, making the last element in the period have the smallest size.

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Most popular questions from this chapter

The first ionization energies of \(\mathrm{Li}, \mathrm{Be}, \mathrm{B}\) and \(\mathrm{C}\) are in the order: (a) \(\mathrm{Li}>\mathrm{Be}<\mathrm{B}<\mathrm{C}\) (b) \(\mathrm{Li}<\mathrm{Be}>\mathrm{B}<\mathrm{C}\) (c) \(\mathrm{Li}>\mathrm{Be}>\mathrm{B}>\mathrm{C}\) (d) \(\mathrm{Li}<\mathrm{Be}>\mathrm{B}>\mathrm{C}\)

Which one of the following electronic configurations corresponds to the most electropositive character? (a) [He]2s? (b) [Ne]3s (c) [Ar]4s (d) [Xe]6s \({ }^{1}\)

Assertion (A): First ionization energy of beryllium is greater than that of boron. Reason (R): Boron has larger size than beryllium. (a) Both \(\mathrm{A}\) and \(\mathrm{R}\) are true and \(\mathrm{R}\) is the correct explanation of \(\mathrm{A}\). (b) Both \(\mathrm{A}\) and \(\mathrm{R}\) are true and \(\mathrm{R}\) is not the correct explanation of \(A\). (c) \(\mathrm{A}\) is true, \(\mathrm{R}\) is false (d) \(\mathrm{A}\) is false, \(\mathrm{R}\) is true

Fill in the blanks. In the periodic table, vertical columns of elements are called ___ and horizontal rows of elements are called ___.

Which of the following elements has maximum electronegativity? (a) \(\overline{\mathrm{P}}\) (b) \(\mathrm{S}\) (c) \(\mathrm{Al}\) (d) \(\mathrm{Si}\)
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