Periodicity

What is the study of repeating patterns in physical or chemical properties in the periodic table called?

Periodicity.

What are the vertical columns of the periodic table known as?

Groups.

What term describes the horizontal rows of the periodic table?

Periods.

Which block of the periodic table contains Group 1 and 2 elements?

s block.

What is the distance between the nucleus and the outermost electrons called?

Atomic radius.

What happens to atomic radius as you move across period 3?

It decreases.

How is electronegativity defined?

The ability of an atom to attract electron density or electrons in a covalent bond.

What is the trend of electronegativity across a period?

It increases from left to right.

What does ionization energy refer to?

The energy required to remove a mole of electrons from a mole of gaseous atoms.

What is the general trend of ionization energy across a period?

It increases.

What factors affect ionization energy?

Distance between electrons and nucleus, and nuclear charge.

How does ionization energy change down a group?

It decreases.

What is the temperature at which a solid turns into a liquid called?

Melting point.

What kind of bond occurs in metals, allowing their outer electrons to move freely?

Metallic bonding.

Which type of bonding involves atoms bonded through strong covalent bonds in structures like silicon?

Giant covalent bonding.

What affects the melting and boiling points of substances?

Type of bonding, strength of forces, and size of particles.

What is the melting point trend for elements in period 3?

It varies based on the type of bonding and forces between particles.

In which region of the periodic table would you find the most electronegative elements?

Top right corner.

What results in higher melting points in substances?

Stronger intermolecular forces.

What characterizes monoatomic bonding as seen in noble gases?

Weak van der Waals forces result in very low melting points.

What are key properties and trends in periodic properties?

Atomic radius decreases across a period, electronegativity increases across a period, and first ionization energy increases across a period.