PVP-AS CHEMISTRY-CHAPTER 10-PERIODICITY 1

Front

What is atomic radius?

Back

The atomic radius is the distance from the nucleus of an atom to the outermost shell of electrons. It generally decreases across a period and increases down a group.

Front

How does atomic radius change across a period?

Back

Atomic radius decreases across a period from left to right due to increased nuclear charge, which pulls electrons closer to the nucleus.

Front

What is ionization energy?

Back

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It generally increases across a period and decreases down a group.

Front

How does ionization energy change down a group?

Back

Ionization energy decreases down a group because the outer electrons are further from the nucleus and experience more shielding from inner electrons.

Front

What is the trend of ionization energy across a period?

Back

Ionization energy increases across a period due to increased nuclear charge, which holds the electrons more tightly.

Front

What is the difference between Mg and Mg²⁺ in terms of size?

Back

Mg²⁺ is smaller than Mg because it loses an energy level when it loses two electrons, resulting in less electron-electron repulsion.

Front

What type of element is nitrogen and how does it behave when forming ions?

Back

Nitrogen is a nonmetal, and it tends to gain electrons when forming an ion, resulting in a negatively charged ion (N³⁻).

Front

What is the relationship between protons and atomic size?

Back

As the number of protons increases, the atomic size generally decreases due to the stronger positive charge attracting electrons more closely to the nucleus.

Front

What is the effect of electron shielding on atomic size?

Back

Electron shielding occurs when inner electrons repel outer electrons, reducing the effective nuclear charge felt by the outer electrons, which can increase atomic size.

Front

Which has a higher ionization energy: N or As?

Back

N has a higher ionization energy than As because N has fewer energy levels, making its valence electrons closer to the nucleus and more strongly attracted.