Question

1. make sure you can name and identify the charge and valence electron for each group.
2. who were the two scientists and what did each do?
3. look over the vocabulary from the notes. write them out again if it helps
4. which element listed below should have chemical properties similar to f? explain.

a. li
b. si
c. br
d. ne

1. know the properties of metals, non- metals, and metalloids
2. answer all of the following for each element

a. f-19
i. period
ii. group number
iii. group name
iv. metal/nonmetal/metalloid
v. block
vi. valence electrons
vii. common ion
viii. protons
ix. neutrons
x. electrons
xi. atomic mass
xii. full electron configuration
b. p-31
i. period
ii. group number
iii. group name
iv. metal/nonmetal/metalloid
v. block
vi. valence electrons
vii. common ion
viii. protons
ix. neutrons
x. electrons
xi. atomic mass
xii. full electron configuration

Explanation:

Question 4 Solution:

Step 1: Recall Chemical Property Rule

Elements in the same group (vertical column) of the periodic table have similar chemical properties because they have the same number of valence electrons. Fluorine (F) is in Group 17 (halogens).

Step 2: Identify Group of Each Option

• a. Li (Lithium) is in Group 1 (alkali metals).
• b. Si (Silicon) is in Group 14 (carbon group).
• c. Br (Bromine) is in Group 17 (halogens), same as F.
• d. Ne (Neon) is in Group 18 (noble gases).

Step 3: Conclude Similarity

Since Br is in the same group as F, they have similar valence electron configurations, leading to similar chemical properties.

Step 1: Determine Atomic Number of F

Fluorine has an atomic number (\(Z\)) of 9 (protons = 9). The mass number (\(A\)) for F - 19 is 19.

Step 1i: Period

The period number is equal to the number of electron shells. F has electron configuration \(1s^2 2s^2 2p^5\), so it has 2 shells. Thus, Period = 2.

Step 1ii: Group Number

F is in Group 17 (halogens). Group number for non - noble gases can also be determined by \(18 - \) number of valence electrons for noble gas - like configuration, but F has 7 valence electrons, and in the modern periodic table, it's Group 17.

Step 1iii: Group Name

Group 17 elements are called Halogens.

Step 1iv: Metal/Nonmetal/Metalloid

Fluorine is a non - metal (it is a gas at room temperature, a poor conductor of heat and electricity, and shows non - metallic properties like forming covalent bonds and gaining electrons).

Step 1v: Block

The valence electrons of F are in the \(p\) - orbital (\(2p^5\)), so it is in the \(p\) - block.

Step 1vi: Valence Electrons

Valence electrons are the outermost electrons. For F, electron configuration is \(1s^2 2s^2 2p^5\), so valence electrons = 7.

Step 1vii: Common Ion

Fluorine gains 1 electron to achieve a stable octet (like Ne's electron configuration), so the common ion is \(F^-\).

Step 1viii: Protons

Protons = atomic number = 9.

Step 1ix: Neutrons

Neutrons (\(N\))=\(A - Z=19 - 9 = 10\).

Step 1x: Electrons (Neutral Atom)

In a neutral atom, electrons = protons = 9. For the ion \(F^-\), electrons = \(9 + 1=10\), but for the neutral F - 19 atom, electrons = 9.

Step 1xi: Atomic Mass

The mass number \(A = 19\), so the atomic mass (approximate, as atomic mass is close to mass number for isotopes) is 19 amu.

Step 1xii: Full Electron Configuration

Using the Aufbau principle, the electron configuration of F (atomic number 9) is \(1s^22s^22p^5\).

Step 1: Determine Atomic Number of P

Phosphorus has an atomic number (\(Z\)) of 15 (protons = 15). The mass number (\(A\)) for P - 31 is 31.

Step 1i: Period

The number of electron shells determines the period. P has electron configuration \(1s^2 2s^2 2p^6 3s^2 3p^3\), so it has 3 shells. Thus, Period = 3.

Step 1ii: Group Number

P is in Group 15 (nitrogen group). The number of valence electrons is 5, and in the modern periodic table, Group 15 elements have 5 valence electrons.

Step 1iii: Group Name

Group 15 elements are called the Nitrogen group (or Pnictogens).

Step 1iv: Metal/Nonmetal/Metalloid

Phosphorus is a non - metal (it exists in various allotropic forms, is a poor conductor of heat and electricity, and shows non - metallic chemical behavior like forming covalent bonds in many compounds).

Step 1v: Block

The valence electrons of P are in the \(p\) - orbital (\(3p^3\)), so it is in the \(p\) - block.

Step 1vi: Valence Electrons

Valence electrons are the outermost electrons. For P, electron configuration is \(1s^2 2s^2 2p^6 3s^2 3p^3\), so valence electrons = 5.

Step 1vii: Common Ion

Phosphorus can gain 3 electrons to achieve a stable octet (like Ar's electron configuration), so a common ion is \(P^{3 - }\) (it can also form other ions in different chemical contexts, but \(P^{3 - }\) is a common anionic form).

Step 1viii: Protons

Protons = atomic number = 15.

Step 1ix: Neutrons

Neutrons (\(N\))=\(A - Z = 31-15 = 16\).

Step 1x: Electrons (Neutral Atom)

In a neutral atom, electrons = protons = 15. For the ion \(P^{3 - }\), electrons = \(15 + 3=18\), but for the neutral P - 31 atom, electrons = 15.

Step 1xi: Atomic Mass

The mass number \(A = 31\), so the atomic mass (approximate, as atomic mass is close to mass number for isotopes) is 31 amu.

Step 1xii: Full Electron Configuration

Using the Aufbau principle, the electron configuration of P (atomic number 15) is \(1s^22s^22p^63s^23p^3\).

Answer:

c. Br (Bromine) should have chemical properties similar to F (Fluorine) because elements in the same group of the periodic table (Group 17 for both F and Br) have the same number of valence electrons, which determines their chemical reactivity and properties.

Question 6a (F - 19) Solution: