How would you calculate the molar mass of 2AgCl?

Write the ionic charges (such as Ca2+) and chemical formulas and fill-in the table below.

Vikentia [17]

1) Lithium and fluorine:

Ionic charges: lithium cation Li⁺ and fluorine anion F⁻.

Chemical formula LiF.

In ionic salt lithium fluoride (LiF), fluorine has electronegativity approximately χ = 4 and lithium χ = 1 (Δχ = 4 - 1; Δχ = 3).

Fluorine attracts electron and it has negative charge and lithium has positive charge.

2) Beryllium and oxygen:

Ionic charges cation Be²⁺ and anion O²⁻.

Chemical formula is BeO.

Beryllium is metal from group 2 and oxygen is nonmetal from group 16.

Electron configuration of beryllium: ₄Be: 1s² 2s², it has two valence electrons in 2s orbital.

Beryllium lose two electrons and to gain electron configuration as noble gas helium (He).

Electron configuration of oxygen atom: ₈O 1s² 2s² 2p⁴.

Oxygen gain two valence electron to form anion with stable electron configuration as noble gas neon (atomic number 10).

3) Magnesium and fluorine:

Ionic charges cation Mg²⁺ and anion F⁻.

Chemical formula is MgF₂.

Magnesium fluoride (MgF₂) is salt, ionic compound.

Magnesium (Mg) is metal from 2. group of Periodic table of elements and has low ionisation energy and electronegativity, which means it easily lose valence electons (two valence electrons).

Magnesium has atomic number 12, which means it has 12 protons and 12 electrons. It lost two electrons to form magnesium cation (Mg²⁺) with stable electron configuration like closest noble gas neon (Ne) with 10 electrons.

Fluorine (F) is nonmetal with greatest electronegativity, which means it easily gain electrons.

Fluorine has atomic number 9, which means it has 9 protons and 9 electrons. It gain one electron to form fluorine anion (F⁻) with stable electron configuration like closest noble gas neon (Ne) with 10 electrons.

4) Aluminum and chlorine:

Ionic charges cation Al³⁺ and anion Cl⁻.

Chemical formula is AlCl₃.

The right name for AlCl₃ is aluminium chloride.

Aluminium chloride is a salt with ionic bonds.

Aluminium (metal from group 13) has oxidation number +3 and chlorine (nonmetal from group 17) has oxidation number -1, chemical compound has neutral charge (+3 + 3 · (-1) = 0).

5) Beryllium and nitrogen:

Ionic charges cation Be²⁺ and anion N³⁻.

Chemical formula is Be₃N₂.

Atomic number of nitrogen is 7, it has 7 protons and 7 electrons.

Electron configuration of nitrogen atom: ₇N 1s² 2s² 2p³.

Nitrogen gain three electrons to form anion with stable electron configuration as noble gas neon (atomic number 10).

4 0

3 years ago

What is the mass in grams of 2.0 moles of NO2

JulsSmile [24]

Molar mass NO₂ = 46.0 g/mol

1 mole -------- 46.0 g
2.0 moles ----- ?

Mass (NO₂) = 2.0 x 46.0 / 1

=> 92.0 g

hope this helps!

8 0

3 years ago

Read 2 more answers

Hi, can someone help me balance this chemistry equation: H2SO4 + RbOH -> Rb2SO4 + H2O

zloy xaker [14]

H2SO4 + 2RbOH -> Rb2SO4 + 2H2O

If you want an explanation, keep reading.

In the first portion, there are two hydrogen ions and four sulfate ions.

The second portion has one rubidium ions and one hydroxide ion.

On the other side of the equation, in order to keep those two rubidiums balanced, you'll need to add a two at the beginning of the second portion, but in that process you are giving a second hydroxide value.

Back to the right side, there is there is water (H2O).

On the first portion, there were two hydrogen ions. The second portion also has two hydroxides because of the value change (adding the two to the front).

So on the fourth portion, you'd have to add another two so you could balance the four hydrogen ions (H2 and 2OH) and the two oxygen ions (2OH).

I hope this was easy to understand.

6 0

3 years ago

Which of the following reactions could be an elementary reaction? 2 NO2(g) + F2(g) → 2NO2F(g) Rate = k[NO2][F2] H2(g) + Br2(g) →

podryga [215]

Answer: The correct answer is $NO(g)+O_2(g)\rightarrow NO_2(g)+O(g);Rate=k[NO][O_2]$

Explanation:

Molecularity of the reaction is defined as the number of atoms, ions or molecules that must colloid with one another simultaneously so as to result into a chemical reaction.

Order of the reaction is defined as the sum of the concentration of terms on which the rate of the reaction actually depends. It is the sum of the exponents of the molar concentration in the rate law expression.

Elementary reactions are defined as the reactions for which the order of the reaction is same as its molecularity and order with respect to each reactant is equal to its stoichiometric coefficient as represented in the balanced chemical reaction.

For the given reactions:

Equation 1: $2NO_2(g)+F_2(g)\rightarrow 2NO_2F(g);Rate=k[NO_2][F_2]$

Molecularity of the reaction = 2 + 1 = 3

Order of the reaction = 1 + 1 = 2

This is not considered as an elementary reaction.

Equation 2: $H_2(g)+Br_2(g)\rightarrow 2HBr(g);Rate=k[H_2][Br_2]^{1/2}$

Molecularity of the reaction = 1 + 1 = 2

Order of the reaction = $1+\frac{1}{2}=\frac{3}{2}$

This is not considered as an elementary reaction.

Equation 3: $NO(g)+O_2(g)\rightarrow NO_2(g)+O(g);Rate=k[NO][O_2]$

Molecularity of the reaction = 1 + 1 = 2

Order of the reaction = 1 + 1 = 2

This is considered as an elementary reaction.

Equation 4: $NO_2(g)+CO(g)\rightarrow NO(g)+CO_2(g);Rate=k[NO_2]^2$

Molecularity of the reaction = 1 + 1 = 2

Order of the reaction = 2 + 0 = 2

In this equation, the order with respect to each reactant is not equal to its stoichiometric coefficient which is represented in the balanced chemical reaction. Hence, this is not considered as an elementary reaction.

Hence, the correct answer is $NO(g)+O_2(g)\rightarrow NO_2(g)+O(g);Rate=k[NO][O_2]$

3 0

3 years ago

Why is it important to conserve or save our energy resources?

earnstyle [38]

answer:

reducing energy use limits the number of carbon emissions in the environment
conserving energy produces a higher quality of life. Reduced emissions result in cleaner air quality
it helps create a healthier planet, or at least helps sustain the resources we already have

explanation:

credits: online research

5 0

3 years ago