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 atomic size generally increases because the outer electrons are held less tightly by the nucleus.

Front

What is nuclear charge?

Back

Nuclear charge is the total charge of the nucleus, which is determined by the number of protons present in the atom.

Front

How does nuclear charge affect ionization energy?

Back

Higher nuclear charge typically leads to higher ionization energy, as the electrons are held more tightly by the nucleus.

Front

What is the trend in atomic radius across a period?

Back

The atomic radius 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 radius down a group?

Back

The atomic radius increases down a group due to the addition of electron shells, which increases the distance between the nucleus and the outermost electrons.

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 are less tightly held.

Front

What is the significance of the periodic table in understanding trends?

Back

The periodic table organizes elements in a way that highlights trends in properties such as atomic size, ionization energy, and electronegativity.

Front

How does electronegativity change across a period?

Back

Electronegativity increases across a period from left to right due to increasing nuclear charge, which attracts bonding electrons more strongly.

Front

What is the trend in electronegativity down a group?

Back

Electronegativity decreases down a group because the increased distance between the nucleus and bonding electrons reduces the nucleus's ability to attract those electrons.