SCH3U September WEEK 3

1

200

as atomic radius of a metal decreases, the reactivity of the metal ________

decreases

300

Elements with a low electronegativity also have a low __________

ionization energy 

400

An element with a large atomic radius is likely to have a ____ electronegativity value

low

500

Rank the following in order of LEAST to MOST electronegative:  F, Ca, Cl, K, Br, 

K, Ca, Br, Cl, F

2

200

This is the term for the minimum energy required to remove the first electron from a neutral atom.

first ionization energy (IE₁)

300

Draw the Lewis structure for PCl3

400

An element with 6 or 7 valence electrons would likely have _____ electronegativity and ____ ionization energy

high;  high

500

Which is the correct structure for SO4 2-? Why?

D because F.C on 2 of the oxygens is -1 and everything else is neutral 

3

200

As atomic radius of a non-metal decreases, the reactivity of a non-metal ______

increases

300

Draw the Lewis structure for CuS

400

_______ increases down a group due to the addition of electron shells, even though the number of protons also increases 

atomic radius 

500

Rank the following in order of MOST to LEAST reactive: P, As, F, Cl, 

F, Cl, P, As

4

200

Why is F the most electronegative element?

Because it has the smallest atomic radius for a non-metal and it only needs to gain 1 e^- to fill its outer shell 

300

This type of element typically has low electronegativity because it tends to donate electrons rather than attract them.

metals 

400

Both O and F are in the same period so why does F have a higher electronegativity?

fluorine has more protons (and therefore a smaller atomic radius), increasing its nuclear pull on valence electrons

500

Removing a third electron from magnesium requires significantly more energy than the first removal because ____

Mg will readily give up 2 electrons in order to have a full outer orbit. However, if a 3rd e^- is removed, now it is removed from a full orbit and this makes Mg very unstable 

5

200

Compared to lithium, sodium has a lower first ionization energy primarily because _______

it has a larger atomic radius and therefore a weaker nuclear pull on the valence e^- (they both only need to lose 1 electron)

300

A chlorine atom will have a much higher second ionization energy than the first because _____

the 2nd e^-  would be removed from a full valence shell which means it will be very unstable 

400

Despite gaining both protons and electrons across a period, atomic radius decreases because ___________

increasing + nuclear pull on the electron orbits 

500

Rank the following in order of MOST to LEAST first ionization energy:  F, He, Cl, Fr, K, 

He, F, Cl, K, Fr