An isotope contains 26 protons, 24 electrons, and 32 neutrons. What is the identity of the isotope

Answer:

Ag(s):H2O(l)  = 3:2

For 3 moles Ag(s) we'll have 2 moles H2O(l)

Option D is correct

Explanation:

Step 1: Balancing the equation

3 Ag (s) + 4 HNO3 (aq) → 3 AgNO3 (aq) + NO (g) + 2 H2O (l)

3Ag(s)  +  4NO  ^3-  +  4H+  →3Ag+ +3NO3- +  +NO  +  2H2O

3Ag(s)  +  NO  ^3-(aq)  +  4H+(aq)  →3Ag+(aq)  +NO(g)  +  2H2O(l)

Step 2: The ratio between Ag(s) and H2O(l)

Ag(s):H2O(l)  = 3:2

For 3 moles Ag(s) we'll have 2 moles H2O(l)

Option D is correct

Answer:

(a) Iron is being oxidized.

(d) Sulfur is being reduced.

Explanation:

Let's consider the following redox reaction.

8 Fe(s) + S₈(s) → 8 FeS(s)

Iron is being oxidized according to the following oxidation half-reaction:

Fe(s) → Fe²⁺(s) + 2 e⁻

Sulfur is being reduced according to the following reduction half-reaction:

S₈(s) + 16 e⁻ → 8 S²⁻(s)

Answer: Formal Charges: Hydrogen = 0 and Oxygen = +1

Unshared Pair of electrons: Hydrogen = 0 and Oxygen = 2

Explanation:

The attachment below shows the Lewis structure and the calculations

Answer:

will be not soluble in water

Explanation:

LiOH is a strong base. Hence it gets completely dissociated in aqueous solution.

is a strong electrolyte. Hence it gets completely dissociated in aqueous solution.

is a strong electrolyte. Hence it gets completely dissociated in aqueous solution.

is a strong electrolyte. Hence it gets completely dissociated in aqueous solution.

is a sparingly soluble salt. Hence it is not dissociated and hence dissolved in water. This is due to the fact that both and ions are similar in size. Hence crystal structure of is quite stable. Hence is reluctant to undergo any dissociation in aqueous solution.

Answer:

p orbitals only

Explanation:

Carbon has an atomic number of 6 so its electron configuration will be 1s² 2s² 2p². It has two orbitals as indicated with the 2 as its period number with the outer orbital have 4 valence electrons. So carbon is in the p-orbital, period 2 and in group 4.

Final answer:

Carbon's valence electrons reside in the 2s and 2p orbitals. These orbitals hybridize during bond formation to create equivalent sp3 hybrid orbitals, as evidenced in the methane molecule. Carbon's valence electrons are not placed in d orbitals.

Explanation:

Carbon (atomic number 6) has a total of six electrons. Two of these fill the 1s orbital. The next two fill the 2s orbital, and the final two are in the 2p subshell. According to Hund's rule, the most stable configuration for an atom is one with the maximum number of unpaired electrons. Therefore, carbon has two electrons in the 2s subshell and two unpaired electrons in two separate 2p orbitals. When discussing valence electrons, the electrons in the outermost shell are the ones considered, which for carbon are the electrons in the second shell namely 2s and 2p.

The geometry of the methane molecule (CH4) illustrates that in the bonding process, the s and p orbitals hybridize to allow the formation of four equivalent bonds with hydrogen atoms. Without hybridization, we would expect three bonds at right angles (from the p orbitals) and one at a different angle (from the s orbital). Nonetheless, through orbital hybridization, all four bonds in methane are identical, which is explained by the concept of sp3 hybridized orbitals.

Therefore, the valence electrons for carbon would be placed in the s orbital and p orbitals, not in the d orbitals, because carbon does not have electrons in the d subshell in its ground state. Additionally, the s and p orbitals are the only ones involved in bonding for carbon in most of its compounds, such as methane.

Learn more about Orbital Placement of Valence Electrons here:

brainly.com/question/14104411

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