Trends Retake Ticket

Front

What is shielding in atomic structure?

Back

Shielding refers to the phenomenon where inner electrons reduce the effective nuclear charge felt by outer electrons, making it easier for them to be removed or to participate in bonding.

Front

How does the shielding effect influence atomic size?

Back

As the shielding effect increases, the outer electrons experience less nuclear attraction, leading to an increase in atomic size.

Front

What is nuclear charge?

Back

Nuclear charge is the total charge of the nucleus, determined by the number of protons present. It influences the attraction between the nucleus and the electrons.

Front

How does nuclear charge affect ionization energy?

Back

Higher nuclear charge generally leads to higher ionization energy, as the increased positive charge attracts electrons more strongly, making them harder to remove.

Front

What is the trend in atomic size across a period?

Back

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

Front

What is the trend in atomic size down a group?

Back

Atomic size increases down a group due to the addition of electron shells, which outweighs the increase in nuclear charge.

Front

What is the relationship between ionization energy and atomic size?

Back

Generally, as atomic size increases, ionization energy decreases because the outer electrons are further from the nucleus and experience less attraction.

Front

What is the significance of comparing elements in the same group?

Back

Elements in the same group have similar chemical properties due to having the same number of valence electrons, which influences their reactivity.

Front

What is the significance of comparing elements in the same period?

Back

Elements in the same period show trends in atomic size, ionization energy, and electronegativity due to increasing nuclear charge.

Front

How does electronegativity change across a period?

Back

Electronegativity increases across a period from left to right as the nuclear charge increases, attracting bonding electrons more strongly.