Question

periodic trends: straw lab

aluminum | al | 13 | 0.143 | 3.84 cm
silicon | si | 14 | 0.117 |
phosphorus | p | 15 | 0.110 |
sulfur | s | 16 | 0.104 |

to calculate the scale factor:
measure the length of a precut straw = 17.7 cm
divide the length of the straw by 2 = 8.85 cm
divide that number by 0.186 = scale factor 47.6 cm

to calculate the length of your straw:
multiply the scale factor by the size of radius given in your data table. answer the following questions in your lab notebook:

1. in a sentence, describe the relationship between atomic number and the size of the atom’s radius going down a group on the periodic table.
2. why does this relationship make sense in relation to what you know about elements on the periodic table?
3. in a sentence, describe the relationship between atomic number and the size of each atom’s radius when going across a period on the periodic table. 4) why does this trend make sense in relation to what you know about the attraction between subatomic particles within the atom?

ionization energy:
the ionization energy for the following elements is estimated to have the following values:

name	symbol	atomic number	ionization energy (kj/mol)	calculated straw length (cm)
magnesium			736
calcium			590
lithium			519
boron			799
carbon			1088
nitrogen			1406

Explanation:

Since the problem here is about answering questions related to periodic trends (atomic radius and ionization energy) which falls under the Natural Science discipline, specifically Chemistry (subfield of Natural Science). Let's take question 1 as an example to answer:

For Question 1 (using Answer - Explanation Format):

When going down a group on the periodic table, as the atomic number increases, the atomic radius generally increases. This is because each subsequent element down a group has an additional electron shell, which increases the distance from the nucleus to the outermost electrons, thus increasing the atomic radius.

Elements in the same group have the same number of valence electrons but different principal energy levels (n). As atomic number increases down a group, a new electron shell (higher n) is added. The outermost electrons are further from the nucleus due to these additional shells, so the atomic radius increases. This aligns with the periodic table's structure where groups are vertical columns with elements having similar valence electron configurations but increasing number of electron shells down the group.

When going across a period on the periodic table, as the atomic number increases, the atomic radius generally decreases. This is because across a period, electrons are added to the same valence shell while protons are added to the nucleus, increasing the nuclear charge which pulls the valence electrons closer to the nucleus, reducing the atomic radius.

Answer:

As the atomic number increases going down a group on the periodic table, the atomic radius of the atom generally increases.

For Question 2 (using Answer - Explanation Format):