Question

regular chemistry
instructions: using your notes, and periodic table answer the following questions.

1. circle the best answer that has the:

a. largest electronegativity
b. largest ionization energy
c. lowest ionization energy
d. smallest atomic radius
e. largest atomic radius
ga ge as sc
o s sc te po
o s se te po
f cl br i at
li na k rb cs

1. for each of the following circle the correct answer

a. metal
b. nonmetal
c. metalloid
d. halogen
e. noble gas
f. transition metal
g. largest atomic number
h. member of alkali metals
i. 6 valence electrons
na p s
li zn o
f al si
cl he b
mg ar ag
k i cu
v zn cs
na mg al
as o br

1. ionization energy

a. define:
b. what is the trend as you move down a group?
c. what is the trend as you move across a period?
d. which family of elements has the highest ionization energy?
e. which family of elements has the lowest ionization energy?
f. arrange the following elements in order of increasing ionization energy: li, o, mg, sr, cl

Explanation:

Step1: Recall periodic - table trends

Electronegativity increases across a period and decreases down a group. Ionization energy increases across a period and decreases down a group. Atomic radius decreases across a period and increases down a group.

Step2: Answer 1a

Among Ga, Ge, As, Sc, the most electronegative is As as it is furthest to the right in the periodic - table among them.

Step3: Answer 1b

No clear list for this part in the question setup, assuming same elements as 1a, As has relatively high ionization energy among them due to its position in the periodic - table.

Step4: Answer 1c

Among O, S, Sc, Te, Po, Sc has the lowest ionization energy as metals generally have lower ionization energies than non - metals and it is a metal among these and furthest down among the metals present.

Step5: Answer 1d

Among O, S, Se, Te, Po, O has the smallest atomic radius as atomic radius increases down a group.

Step6: Answer 1e

Among F, Cl, Br, I, At, At has the largest atomic radius as atomic radius increases down a group.

Step7: Answer 2a

Na is a metal.

Step8: Answer 2b

P and S are non - metals.

Step9: Answer 2c

Si is a metalloid.

Step10: Answer 2d

F and Cl are halogens.

Step11: Answer 2e

He is a noble gas.

Step12: Answer 2f

Ag and Cu are transition metals.

Step13: Answer 2g

Cs has the largest atomic number among the given elements (55 for Cs, 19 for K, 23 for V, 30 for Zn).

Step14: Answer 2h

Na and Cs are members of alkali metals.

Step15: Answer 2i

O and Te have 6 valence electrons.

Step16: Answer 3a

Ionization energy is the energy required to remove an electron from a gaseous atom or ion.

Step17: Answer 3b

As you move down a group, ionization energy decreases because the outermost electrons are further from the nucleus and are less tightly held.

Step18: Answer 3c

As you move across a period, ionization energy increases because the effective nuclear charge increases and the atomic radius decreases, making it harder to remove an electron.

Step19: Answer 3d

Noble gases have the highest ionization energy in each period because they have a full valence shell and are very stable.

Step20: Answer 3e

Alkali metals have the lowest ionization energy in each period as they have one valence electron which is easily removed.

Step21: Answer 3f

The order of increasing ionization energy for Li, O, Mg, Sr, Cl is Sr < Li < Mg < O < Cl. This is based on the periodic trends of ionization energy (decreases down a group and increases across a period).

Answer:

1a. As
1b. As (assuming same elements as 1a)
1c. Sc
1d. O
1e. At
2a. Na
2b. P, S
2c. Si
2d. F, Cl
2e. He
2f. Ag, Cu
2g. Cs
2h. Na, Cs
2i. O
3a. The energy required to remove an electron from a gaseous atom or ion.
3b. Decreases.
3c. Increases.
3d. Noble gases.
3e. Alkali metals.
3f. Sr < Li < Mg < O < Cl