Ionization Energy and Atomic Trends Quiz

What does 1st ionization energy measure?

• Adding an electron

• Removing the outermost electron

• Size of the atom

• Adding a proton

Answer explanation

1st ionization energy measures the energy required to remove the outermost electron from an atom. This process reflects how easily an atom can lose an electron, making 'removing the outermost electron' the correct choice.

1st ionization energy is the energy needed to:

• Add an electron to a neutral atom

• Remove the outermost electron from a neutral atom

• Change the nucleus

• Add a neutron

Answer explanation

1st ionization energy refers to the energy required to remove the outermost electron from a neutral atom, making it positively charged. This process is essential in understanding atomic behavior and reactivity.

Valence electrons are found in:

• The innermost shell

• The outermost shell

• The nucleus

• None

Answer explanation

Valence electrons are located in the outermost shell of an atom. These electrons are crucial for chemical bonding and determine the reactivity of the element.

Which electrons participate in bonding with other atoms?

• Core electrons

• Valence electrons

• Inner electrons

• None

Answer explanation

Valence electrons are the outermost electrons of an atom and are primarily responsible for forming bonds with other atoms. Core and inner electrons are not involved in bonding.

What does electron shielding refer to?

• Electrons blocking the nucleus charge

• Adding electrons to an atom

• Removing electrons

• None

Answer explanation

Electron shielding refers to the phenomenon where inner electrons block the attractive force of the nucleus on outer electrons. This makes it easier for outer electrons to exist at higher energy levels, hence the correct choice is 'Electrons blocking the nucleus charge'.

Electron shielding occurs due to:

• Outer electrons blocking inner electrons

• Inner electrons blocking outer electrons

• Electrons moving to higher energy levels

• None

Answer explanation

Electron shielding occurs when inner electrons block the attraction between the nucleus and outer electrons, reducing the effective nuclear charge felt by the outer electrons. Thus, the correct answer is 'Inner electrons blocking outer electrons'.

Energy levels and electron shielding are connected because:

• Lower energy levels block nuclear charge

• Higher energy levels block inner electrons

• Both are unrelated

• None

Answer explanation

Lower energy levels, being closer to the nucleus, effectively shield outer electrons from the full nuclear charge. This shielding reduces the effective nuclear charge felt by outer electrons, influencing their energy levels.

Electron shielding is caused by:

• Electrons in lower energy levels

• Protons in the nucleus

• Neutrons in the nucleus

• None

Answer explanation

Electron shielding occurs when electrons in lower energy levels repel outer electrons, reducing the effective nuclear charge felt by them. This makes 'Electrons in lower energy levels' the correct choice.

Across a period, ionization energy:

• Increases

• Decreases

• Stays the same

• Both

Answer explanation

Across a period, ionization energy increases due to the greater nuclear charge attracting electrons more strongly, making it harder to remove an electron. Thus, the correct answer is 'Increases'.

Down a family, ionization energy:

• Increases

• Decreases

• Stays the same

• Both

Answer explanation

Down a family, ionization energy decreases due to increased atomic size and shielding effect, making it easier to remove an electron. Thus, the correct answer is 'Decreases'.