5) Periodic Trends Pt.1

What is atomic radius?

The distance between the nucleus and the outer edge of the electron cloud

What is the distance between the nucleus and the outer edge of the electron cloud?

the atomic radius

What is ionization energy?

the amount of energy required to remove the first valence electron from an atom

What is the amount of energy required to remove the first valence electron?

ionization energy

What is electronegativity?

the ability of an atom to attract electrons in another atom to fill its valence shell

What is the ability of an atom to attract electrons in another atom to fill its valence shell?

electronegativity

What is shielding?

the net positive charge felt by the negative valence electrons after taking into account the affect of shielding electrons

What is the net positive charge felt by the negative valence electrons after taking into account the affect of shielding electrons?

shielding

What is coulombic attraction?

the attraction between positive and negative charges

What is the attraction between positive and negative charges?

coulombic attraction

Does coulombic attraction increase or decrease as the charges increase?

increase

Does charge increase or decrease as coulombic attraction increase?

increase

Does coulombic attraction increase or decrease as the distance between them increases?

decrease

Does the distance increase or decrease as coulombic attraction decreases?

increase

Coulombic attraction formula

charge (q1xq2) / distance between charged particles (r²)

charge (q1xq2) / distance between charged particles (r²)

coulombix attraction formula

Why does coulombic attraction increase from left to right?

because the number of protons increases

Because the number of protons increases, coulombic attraction _

increases from left to right

Coulombic attraction decreases down a group because the

the distance between the positive nucleus and the negative valence electrons increases

Because the distance between the positive nucleus and the negative valence electrons increases, coulombic attraction

decreases down a group

Atomic size increases from right to left across a period because

decreased number of protons, less attraction, larger atom

Because of a decreased number of protons, less attraction, and a large atom, atomic size

increases from right to left

Atomic size increases from top to bottom within a group because

increased number of energy levels, increased distance, less attraction

Because of an increased number of energy levels, increased distance, and less attraction, atomic size

increases from top to bottom of a group

Ionization energy increases from left to right across a period because

increased number of protons, increased attraction, more energy required

Because of an increased number of protons, increased attraction, and more energy required, ionization energy

increases from left to right across a period

Ionization energy increases from bottom to top within a group because

fewer energy levels, less distance, more attraction, more energy required

Because of fewer energy levels, less distance, more attraction, and more energy required, ionization energy

increases from bottom to top

Electronegativity increases from left to right across a period because

increased number of protons, increased attraction

because of an increased number of protons, and increased attraction, electronegativity

increases from left to right

Electronegativity increases from bottom to top within a group because

fewer energy levels, increased attraction, smaller atomic size, stronger pull on electrons on another atom

Because of fewer energy levels, increased attraction, smaller atomic size, and a stronger pull on electrons on another atom, electronegativity

increases from bottom to top within a group