4. which subatomic particle is most responsible for the current arrangement of elements on the periodic table?
5. which subatomic particle is most responsible for the chemical properties of an element?
6. what is similar about all of the elements in the same group?
7. horizontal rows are ______ and vertical columns are ______ or ______.
8. fill in the following chart:
| group number | name of the group | reactivity of all elements in group | valence electrons |
| --- | --- | --- | --- |
| 1 | | | |
| 2 | | | |
| 3-12 | n/a | n/a | |
| 13 | n/a | n/a | |
| 14 | n/a | n/a | |
| 15 | n/a | n/a | |
| 16 | n/a | n/a | |
| 17 | | | |
| 18 | | | |
9. where are the metals located on the periodic table? where are the non-metals located? the metalloids? what are some properties of metals? metalloids? nonmetals?
10. how many total electrons fit in an s sublevel? ____ p? ____ d? ____ f? ____
11. what do all elements in the same group have the same number of?
12. what do all elements in the same period have the same number of?

Question

4. which subatomic particle is most responsible for the current arrangement of elements on the periodic table?
5. which subatomic particle is most responsible for the chemical properties of an element?
6. what is similar about all of the elements in the same group?
7. horizontal rows are ______ and vertical columns are ______ or ______.
8. fill in the following chart:
| group number | name of the group | reactivity of all elements in group | valence electrons |
| --- | --- | --- | --- |
| 1 |  |  |  |
| 2 |  |  |  |
| 3-12 | n/a | n/a |  |
| 13 | n/a | n/a |  |
| 14 | n/a | n/a |  |
| 15 | n/a | n/a |  |
| 16 | n/a | n/a |  |
| 17 |  |  |  |
| 18 |  |  |  |
9. where are the metals located on the periodic table? where are the non-metals located? the metalloids? what are some properties of metals? metalloids? nonmetals?
10. how many total electrons fit in an s sublevel? ____ p? ____ d? ____ f? ____
11. what do all elements in the same group have the same number of?
12. what do all elements in the same period have the same number of?

Accepted Answer

### Question 4
# Brief Explanations:
The periodic table is arranged by atomic number, which is the number of protons in an atom's nucleus. Protons determine the element's identity and the order in the periodic table.
# Answer:
Proton

### Question 5
# Brief Explanations:
Chemical properties are determined by how an atom interacts with other atoms, which is mainly due to the number of valence electrons (electrons in the outermost shell). Electrons are involved in bonding and chemical reactions.
# Answer:
Electron (specifically valence electrons)

### Question 6
# Brief Explanations:
Elements in the same group (vertical column) have the same number of valence electrons. This similar electron configuration leads to similar chemical properties (e.g., reactivity patterns, ability to form certain bonds).
# Answer:
Same number of valence electrons (and thus similar chemical properties)

### Question 7
# Brief Explanations:
In the periodic table, horizontal rows are called periods. Vertical columns are called groups (or families). This is standard periodic table terminology.
# Answer:
Horizontal rows are $\boldsymbol{\text{periods}}$ and vertical columns are $\boldsymbol{\text{groups}}$ or $\boldsymbol{\text{families}}$.

### Question 8
To fill the chart:

| Group number | Name of the group       | Reactivity of all elements in group | Valence Electrons |
|--------------|-------------------------|--------------------------------------|-------------------|
| 1            | Alkali Metals           | Highly reactive (increases down)     | 1                 |
| 2            | Alkaline Earth Metals   | Reactive (increases down)            | 2                 |
| 3 - 12       | Transition Metals       | N/A (varies, less reactive than 1/2) | Varies (d - block) |
| 13           | Boron Group             | N/A (moderate reactivity)            | 3                 |
| 14           | Carbon Group            | N/A (varies, C is stable, others vary) | 4                 |
| 15           | Nitrogen Group          | N/A (varies, N is reactive, P etc. vary) | 5                 |
| 16           | Chalcogens              | N/A (O is reactive, S etc. vary)     | 6                 |
| 17           | Halogens                | Highly reactive (decreases down)     | 7                 |
| 18           | Noble Gases             | Non - reactive (inert)               | 8 (except He: 2)  |

### Question 9
#### Location:
- **Metals**: Most are located on the left - hand side and in the middle of the periodic table (except for hydrogen). They occupy groups 1 - 2 (s - block) and 3 - 12 (d - block) and some of group 13 - 16 (p - block metals like Al).
- **Non - metals**: Located on the right - hand side of the periodic table, mainly in groups 14 - 18 (p - block), with hydrogen also being a non - metal on the left.
- **Metalloids**: Found along the "staircase" line that separates metals and non - metals, including elements like B, Si, Ge, As, Sb, Te, Po.

#### Properties:
- **Metals**: Good conductors of heat and electricity; malleable (can be hammered into sheets) and ductile (can be drawn into wires); have a shiny (metallic) luster; generally have high melting and boiling points (except for some like Hg which is liquid at room temp).
- **Metalloids**: Have properties intermediate between metals and non - metals. They are semi - conductors (conduct electricity better than non - metals but worse than metals); have a somewhat metallic or non - metallic appearance depending on the element.
- **Non - metals**: Poor conductors of heat and electricity (except for graphite, a form of carbon); are brittle in solid form; have lower melting and boiling points (many are gases at room temp like O, N, F, Cl; some are solids like C, P, S; one is liquid - Br); do not have a metallic luster.

### Question 10
# Explanation:
## Step1: s sublevel
The s sublevel has 1 orbital, and each orbital can hold a maximum of 2 electrons. So, the number of electrons in an s sublevel is $2\times1 = 2$.
## Step2: p sublevel
The p sublevel has 3 orbitals. Since each orbital holds 2 electrons, the number of electrons in a p sublevel is $2\times3=6$.
## Step3: d sublevel
The d sublevel has 5 orbitals. So, the number of electrons in a d sublevel is $2\times5 = 10$.
## Step4: f sublevel
The f sublevel has 7 orbitals. Thus, the number of electrons in an f sublevel is $2\times7=14$.
# Answer:
s: $2$, p: $6$, d: $10$, f: $14$

### Question 11
# Brief Explanations:
Elements in the same group (vertical column) have the same number of valence electrons. Valence electrons are the electrons in the outermost energy level and determine the chemical behavior of the element.
# Answer:
Number of valence electrons

### Question 12
# Brief Explanations:
Elements in the same period (horizontal row) have the same number of electron shells (energy levels). For example, all elements in period 2 have electrons in 2 energy levels (n = 2).
# Answer:
Number of electron shells (energy levels)

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