Answer:
3.73 g of Li.
Explanation:
What is given?
Volume of hydrogen gas, H2 (V) = 6.00 L.
Pressure (P) = 1.10 atm.
Temperature (T) = 25.0°C + 273 = 298 K.
R = 0.082 L*atm/mol*K.
Step-by-step solution:
First, we have to find the number of moles of hydrogen gas (H2) using the ideal gas formula:
[tex]PV=nRT,[/tex]where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant and T is the temperature on Kelvin scale. So let's solve for 'n' and replace the given values:
[tex]n=\frac{PV}{RT}=\frac{1.10\text{ atm}\cdot6.00\text{ L}}{0.082\text{ }\frac{L\cdot atm}{mol\cdot K}\cdot298K}=0.270\text{ moles.}[/tex]Based on this, we have 0.270 moles of H2.
You can see in the chemical equation that 2 moles of Li reacted produce 1 mol of H2, so we have to state a rule of three:
[tex]\begin{gathered} 2\text{ moles Li}\rightarrow1\text{ mol H}_2 \\ ?\text{ moles Li}\rightarrow0.270\text{ moles H}_2 \end{gathered}[/tex]The calculation will look like this:
[tex]0.270\text{ moles H}_2\cdot\frac{2\text{ moles Li}}{1\text{ mol H}_2}=0.540\text{ moles Li.}[/tex]The final step is to convert 0.540 moles of Li to grams using its molar mass that can be found in the periodic table, which is 6.9 g/mol:
[tex]0.540\text{ moles Li}\cdot\frac{6.9\text{ g Li}}{1\text{ mol Li}}=3.73\text{ g Li.}[/tex]The answer is that we must use 3.73 g of Li to produce 6.00 L of H2 at 1.10 atm and 25.0 °C.
Use the equation: 3H2, + N2 —-2NH3, (all are gasses)If you need to make 467L of ammonia gas, how many grams of nitrogen gás do you need to start with?
1) First, let's rewrite the equation:
3 H2 + N2 ---> 2 NH3
If you need to make 467 L ammonia gas (NH3), let's find out how many moles of it do we need.
For this, we use the molar volume of gases: 22.4L/mol
So:
467 L ------ x mol
22.4 L ----- 1 mol
22.4x = 467
x = 20.8 mol of NH3
2) Now we use the proportion of the chemical equation to find out the quantity in moles of N2 (nitrogen gas):
1 mol of N2 ---- 2 mol of NH3
x mol of N2 ----- 20.8 mol of NH3
2x = 20.8
x = 10.4 mol of N2
3) Now we use the molar mass of N2 to find the quantity in grams that we need to start with:
molar mass N2 = 2x14 = 28 g/mol
Now we use the following equation:
mass = mole × molar mass
mass = 10.4 × 28 = 291.2 grams of Nitrogen Gas
Answer: 291.2 grams of Nitrogen Gas
why do engineers come up with as many ideas to solve a problem as possible?
Engineers come up with as many ideas to solve a problem as possible is so as to choose the best which is applicable in helping people.
Who is an Engineer?This is referred to as an individual or a professional which employs the use of scientific knowledge in the construction and building of different types of machines and tools.
An engineer is someone who has a good analytic and problem solving skills and comes up with many ideas so as to be able to choose the best from the set of alternatives in helping people solve their problems or issues.
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CaCO3(s) + 2HCl(aq) ---> CaCl2(s) + CO2(g) + H2O(ℓ)What would be the volume of CO2 (at STP) produced from the complete reaction of 10.0 grams of CaCO3?
The equation is balanced since the number of atoms of each element is the same on each side of the reaction.
Now, we will calculate the number of moles present in 10 grams of CaCO3. We will use the molar mass of CaCO3 for this
[tex]\begin{gathered} lesofCaCO3=gCaCO_3\times\frac{1molCaCO_3}{MolarMass,\text{gCaCO}_3} \\ MolesofCaCO3=10.0gCaCO_3\times\frac{1molCaCO_3}{100.0869gCaCO_3}=0.1molCaCO_3 \end{gathered}[/tex]Assuming that the rest of the reactants are in excess, 0.1 mol of CaCO3 will react and form 0.1 mol of CO2, since the ratio is 1 to 1.
Now to calculate the volume, we can apply the ideal gas law which tells us:
[tex]PV=nR_{}T[/tex]Where,
P is the pressure (STP) =1 atm
V is the volume in Liters
n is the number of moles = 0.1 mol CO2
R is a constant = 0.08206 (atm L)/(mol K)
T is the temperature (STP)= 273.15K
Now, we clear the volume and write the known values:
[tex]\begin{gathered} V=\frac{nR_{}T}{P} \\ V=\frac{0.1\text{mol}\times0.08206\frac{atm.L}{mol.K}\times273.15K}{1atm} \\ V=2.2L \end{gathered}[/tex]The volume of CO2(at STP) produced would be 2.2L
How many grams are in 4.02 x 10^21 atoms of calcium?
0.268grams
Explanations:According to the Avogadro's constant
1 mole of an atom = 6.02 * 10^23 molecules
Given the following
atoms of calcium = 4.02 x 10^21 atoms
Determine the moles of calcium
[tex]\begin{gathered} moles\text{ of Ca}=\frac{4.02\times10^{21}}{6.02\times10^{23}} \\ moles\text{ of Ca}=0.668\times10^{21-23} \\ moles\text{ }of\text{ Ca}=0.668\times10^{-2} \\ moles\text{ of Ca}=0.00688moles \end{gathered}[/tex]Determine the mass of Calcium
[tex]\begin{gathered} Mass=mole\times molar\text{ mass} \\ Mass=0.00688\times40.078 \\ Mass\text{ of Ca}=0.268gram \end{gathered}[/tex]Hence the required grams in 4.02 x 10^21 atoms of calcium is 0.268grams
I’m having trouble figuring out how to do number 13. Iv done some things but still cannot seem to figure it out.
This is a stoichiometry problem, where we have an initial amount of reactant and we need to find out how much of the product will we end up with, in order to do that we need to:
1. Set up the properly balanced equation, which the question already provided us
2 KClO3 -> 2 KCl + 3 O2
2. Check the molar ratio between the two compounds, which is 2:3, 2 moles of KClO3 will produce 3 moles of O2, but we have 3 moles of KClO3
2 KClO3 = 3 O2
3 KClO3 = x O2
x = 4.5 moles of O2 will be produced from 3 moles of KClO3
3 KClO3
2 KClO3/ 3 O2
4.5 O2
Calculate the molar mass of NaHCO3 and round it to 2 decimal places.
To calculate the molar mass of NaHCO₃, we need to add the molar mass of each of its atoms.
This compound has 1 atom of Na, 1 of H 1 of C and 3 of O.
The molar mass of these atoms can be consulted on a periodic table, and they are:
[tex]\begin{gathered} M_{Na}=22.9898g/mol \\ M_H=1.0079g/mol \\ M_C=12.0107g/mol \\ M_O=15.9994g/mol \end{gathered}[/tex]So, the molar mass of NaHCO₃ is:
[tex]\begin{gathered} M_{NaHCO_3}=1\cdot M_{Na}+1\cdot M_H+1\cdot M_C+3\cdot M_O \\ M_{NaHCO_3}=(1\cdot22.9898+1\cdot1.0079+1\cdot12.0107+3\cdot15.9994)g/mol \\ M_{\mleft\{NaHCO_3\mright\}}=\mleft(22.9898+1.0079+12.0107+47.9982\mright)g/mol \\ M_{\mleft\{NaHCO_3\mright\}}=84.0066g/mol\approx84.01g/mol \end{gathered}[/tex]6. What is the percent composition of chlorine in calcium chloride, CaCl₂?a. 32%b. 36%c. 50%d. 64%
The first step we have to follow is to find the molecular mass of CaCl2.
[tex]\begin{gathered} Ca=40\times1=40 \\ Cl_2=35.45\times2=70.9 \\ CaCl_2=40+70.9=110.9 \end{gathered}[/tex]Finally divide the mass of Cl2 by the mass of CaCl2 and multiply this product times 100:
[tex]\frac{70.9}{110.9}\cdot100=63.93[/tex]It means that the correct answer is 64%.
Atom A and B both have 10 protons A have 10 B has 11 neutrons, which statement is true A,b have the same element, theyvhave differnet elements, if they have the same mass, only atom b is a isotope
Atom A and B both have 10 protons A have 10 B has 11 neutrons is A and B are isotopes of same element.
Isotopes are the atoms of same elements , that has same number of proton but different number of neutrons , mass no. is depends on neutrons present in an atom. the given situation is :
number of proton number of neutron
Atom A 10 10
Atom B 10 11
Isotopes are the members of the same family of same elements.
Thus, Atom A and B both have 10 protons A have 10 B has 11 neutrons is A and B are isotopes of same element.
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Which of the following is a conclusion that the student can draw based on these observations? The two clear liquids-
In the process that they describe to us, a mixture initially occurs between these two liquids, when they are mixed, a chemical reaction occurs and one of the products obtained is not soluble in the liquids, therefore a precipitate will form. This type of reaction is called a precipitation reaction.
Therefore, the answer will be:
C) Have gone through a chemical reaction in which a new substance called a precipitate was produced
Aluminum bromide can be prepared by reacting small pieces of aluminum foil with liquid bromine at room temperature. The balanced chemical reaction is:2Al(s) + 3Br2(l) → 2AlBr3(s)How many moles of Br2 are needed to produce 5 mol of AlBr3, if sufficient Al is present?
Based on the mole ratio from the chemical reaction 3 moles of Br2 produces 2 moles of AlBr3. We can set this equation up to determine the unknown:
[tex]\begin{gathered} \frac{2}{3}=\frac{x}{5} \\ 3x=2\times5 \\ x=\frac{10}{3} \\ x=3.3moles \end{gathered}[/tex]3.3 moles of Br2 is needed to reacts with 5 mol of AlBr3.
When atoms become bonded with covalent bonds, the result is called a(n):A. ionic bond.B. ion.C. valence.D. molecule.SUBMIT
Explanation:
A covalent bond occurs when electrons are shared by atoms. Atoms will covalently bond with other atoms to gain stability.
A group of atoms held together by covalent bonds is called a molecule.
Answer: D. molecule
10.The drink mix and water in a drink solution can be separated by...Select one:a. filtering out the drink mix from the water.b. evaporating the water.c. picking out the drink crystals by hand.d. drawing the drink crystals out with a magnet.
Answer
b. evaporating the water.
Explanation
The ingredients in a solution cannot be separated by hand because of changes in the ingredients' physical properties. But evaporation can be used to separate some solutions. For example, just in the case of the drink mix and water in a drink solution given.
31.The correct name for the compound that has the formula BaCl2 is...Select one:a. Baride chlorine.b. Barium chloride.c. Barium chlorine.d. Barium chlorite.
ANSWER
option B
EXPLANATION
Given that;
The molecular formula of the compound is given as BaCl2
The compound contain a metal and a non-metal
Ba means Barium
Cl2 is chloride because its a diatomic gas
Then BaCl2 is called Barium chloride
Therefore, the correct answer is option B
2.Solid iron combines with oxygen gas to form solid iron(III) oxide. Which of the following equations best describes this reaction?Select one:a. Ab. Bc. Cd. D
ANSWER
option B
EXPLANATION;
The chemical symbol of iron is Fe
The chemical symbol of oxygen is O2
[tex]\text{ 4Fe + 3O}_2\text{ }\rightarrow\text{ 2Fe}_2O_3[/tex]Therefore, the correct answer is B
How do you figure this question out in CHEM 101?What is the mass in grams are in 5.32x10^22 molecules of CO2?
To answer this question, the first step is to convert the given number of molecules to moles using Avogadro's number:
[tex]5.32\times10^{22}molecules\cdot\frac{1molCO_2}{6.022\times10^{23}molecules}=0.088molCO_2[/tex]Now, use the molecular weight of CO2 to find the mass of this amount of moles:
[tex]0.088molCO_2\cdot\frac{44g}{molCO_2}=3.872g[/tex]The mass of 5.32x10^22 molecules of CO2 is 3.872g.
I need help on #5-#7
If 5750 J of energy are added to 455 g of granite at 24 °C. The final temperature of granite is 39.9 °C
Given that :
heat energy = 5750 J
mass of granite = 455 g
initial temperature = 24 °C
specific heat capacity = 0.12 cal / g °C = 0.790 J/ g °C
the expression for the heat capacity is given as :
Q = mcΔT
5750 J = 455 g × 0.790 J/ g °C ( T - 24 °C)
5750 = 359.45 T - 8626.8
T = 39.9 °C
if 5750 J of energy are added to 455 g of granite at 24 °C. The final temperature of granite is 39.9 °C
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Neon (Z=10) has the minimum electron affinity in the 2nd period in the periodic tableIs it true or false? And why?
ANSWER
False
EXPLANATION
Electron affinity is defined as the energy released by adding an electron to an isolated gaseous atom
Neon has the electronic configuration of 2, 8, This implies that it belongs to period 2 and group 8
Recall, that Neon is a noble gas. Noble gases do not accept or release electrons.
Hence, neon does not have the tendency to accept or release electrons.
Neon as a noble gas has a large positive value for electron affinity
Therefore, the statement is not TRUE
Perform the following operationand express the answer inscientific notation.5.4x103 x 1.2x107[ ? ]x10[?]Coefficient (green) Exponent (yellow)tCoefficient (green)Enter
Since the operation is a multiplication, the order in which we made the multiplications doesn't matter, so we can reoprder it:
[tex]5.4\times10^3\times1.2\times10^7=5.4\times1.2\times10^3\times10^7[/tex]Now, we calculate each of them:
[tex]6.48\times10^{3+7}=6.48\times10^{10}[/tex]Oxygen gas is made up of diatomic non-polar covalent molecules. This leads to very weak attraction between molecules. Which statement would this best support?
The oxygen gas is non polar because there is no interaction between the molecules of the gas.
What is a diatomic molecule?A diatomic molecule is one that has only two atoms in it. These atoms are usually atoms of the same element in the majority of the cases that we encounter. Given the fact that the both atoms belong to the same substance, the electronegativity difference between the atoms is zero.
Given that the electronegativity difference between the atoms is zero, there is little or no interaction between the molecules of the substance. Thus the very weak intermolecular interaction is coming from the fact that there is no kind of interaction between the molecules.
Thus oxygen gas is covalent and the molecules do not interact with each other because the bond is nonpolar.
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How many grams of H3PO4 could be produced from 94 g of H2O and 186 g of PCL5 according to the equation below?
Answer:
[tex]89.4\text{ g of H}_3PO_4[/tex]Explanation:
Here, we want to get the mass of H3PO4 produced
We start by getting the balanced equation of reaction:
[tex]PCl_5\text{ + 4H}_2O\text{ }\rightarrow\text{ 5HCl + H}_3PO_4[/tex]The mass of H3PO4 produced would be based on the limiting reactant
The limiting reactant here is the one that would produce less amount of the product H3PO4
Firstly, let us get the number of moles of H3PO4 produced by each of the reactants
To get this, we start by getting the number of moles of each that reacted
We get this by dividing the masses by the molar masses
For water, we have it that the molar mass is 18 g/mol
Thus, the number of moles would be:
[tex]\frac{94}{18}\text{ = 5.2 moles}[/tex]From the balanced equation of reaction:
4 moles of water produced 1 mole of H3PO4
5.2 moles of water will produce x moles of H3PO4
Thus:
[tex]\begin{gathered} x\text{ }\times4\text{ = 5.2}\times1 \\ x\text{ = }\frac{5.2}{4}\text{ = 1.3 mole} \end{gathered}[/tex]For PCl5
The molar mass is 208 g/mol
Thus,we have the number of moles as:
[tex]\frac{186}{208}\text{ = 0.894 mol}[/tex]From the equation of reaction:
1 mol of PCl5 produced 1 mol of H3PO4
That means 0.894 mol of PCl5 produced 0.894 mol of H3PO4
Since PCl5 produced a lesser amount of moles of water, that means, it is the limiting reactant
To get the mass of H3PO4 produced, we multiply this number of moles by
the molar mass of H3PO4
The molar mass of H3PO4 is 100 g/mol
Thus, we have the mass of H3PO4 produced as:
[tex]0.894\text{ }\times\text{ 100 = 89.4 g}[/tex]what would be the effect on the melting point of a sample if it were not dried completely after filtering the recrystallized sample?
It can lower and expand the melting point if the sample is not dried completely.
Impurities may be present in a sample if the drying process is not complete. The melting point is decreased and widened when contaminants are still present in a sample. For instance, if a substance's usual melting point range is 104C to 106C, improper drying could result in the presence of impurities, which would lower and widen the melting point range to something like 85C to 97C.
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What physical property can help characterize fragments of glass at a crime scene?
A.
flammability
B.
toxicity
C.
density
D.
volume
Answer:
I believe it is
C. density
Explanation:
have a nice day!❀
during the decomposition of 34 gr ammonia into nitrogen and hydrogen 92 KJ are absorbed. How many grams of ammonia are decomposed when 184 KJ are absorbed? write the decomposition reaction
Explanation:
Ammonia will decompose into nitrogen gas and hydrogen gas according to the following reaction. In that reaction 92 kJ will be absorbed.
2 NH₃ ----> N₂ + 3 H₂ ΔH = 92 kJ
Since the heat is absorbed, the sign is positive and we can add it to the reactants side.
2 NH₃ + 92 kJ ----> N₂ + 3 H₂
When 92 kJ are absorbed 34 g of ammonia are reacted. We can use that relationship to find the mass of ammonia that reacted when 184 kJ where absorbed.
34 g of NH₃ : 92 kJ
mass of NH₃ = 184 kJ * 34 g of NH₃/(92 kJ)
mass of NH₃ = 68 g
Answer: 68 g of ammonia were decomposed.
2 NH₃ ----> N₂ + 3 H₂ ΔH = 92 kJ
Determine the [H+] of a solution that has a [OH-] of 6.25*10-12. (Enter answer in expanded format not scientific notation)
answer and explanation
we are given the [OH] concentration as 6.25*10-12
and we know that
[H+][OH-] = 1.0*10^-14
an so using this relationship we can determine the [H+]
[H+][6.25*10-12] = 1.0*10-14
[H+] = 0.0016M
Identify the equation with the elements in BeSO4 in their standard state as the reactants and BeSO4 as the product.
Answer:
[tex]E[/tex]Explanation:
Here, we want to identify the elements in BeSO4 in their standard state as the reactants and BeSO4 as the product
From what we have, there are 4 atoms of oxygen, 1 atom of Beryllium, and 1 atom of sulfur
In their standard state, oxygen is a gas, Berrylium and Sulfur are solids
The number of elements atom on the reactant side must be equal to that on the product side
Thus, we have the correct choice of answer as E
You have 6.0 g of C2H6 and 20.0 g of O2 for a combustion reaction. If you actuallyproduce 3.80 g of CO2 , What is the percent yield?
Answer:
The percent yield is 24.2%.
Explanation:
1st) It is necessary to balance the chemical reaction:
[tex]2C_2H_6+7O_2\rightarrow4CO_2+6H_2O[/tex]2nd) From the balanced reaction, we know that 2 moles of C2H6 react with 7 moles of O2 to produce 4 moles of CO2. With the molar mass of C2H6 (30g/mol), O2 (32g/mol) and CO2 (44g/mol), we can convert the moles to grams:
- C2H6 conversion:
[tex]2moles*\frac{30g}{1mole}=60g[/tex]- O2 conversion:
[tex]7moles*\frac{32g}{1mole}=224g[/tex]-CO2 conversion:
[tex]4moles*\frac{44g}{1mole}=176g[/tex]Now we know that 60g of C2H6 react with 224g of O2 to produce 176g of CO2.
3rd) From the given values of C2H6 (6.0g) and O2 (20.0g), it is necessary to find out which one is the limiting reactant and which one is the excess reactant:
[tex]\begin{gathered} 60gC_2H_6-224gO_2 \\ 6.0gC_2H_6-x=\frac{6.0gC_2H_6*224gO_2}{60gC_2H_6} \\ x=22.4gO_2 \end{gathered}[/tex]We can see that the 6.0g of C2H6 will need 22.4g of O2 to react, but we only have 20.0g of O2, so O2 is the limiting reactant and C2H6 will be the excess reactant.
4th) Now, using the limiting reactant, we have to calculate the grams of CO2 that should be produced from the stoichiometry of the reaction (this is the Theoretical yield):
[tex]\begin{gathered} 224gO_2-176gCO_2 \\ 20.0gO_2-x=\frac{20.0gO_2*176gCO_2}{224gO_2} \\ x=15.7gCO_2 \end{gathered}[/tex]5th) Finally, we can calculate the Percent yield of the reaction, by using the Theoretical yield (15.7g) and the Actual yield (3.80g):
[tex]\begin{gathered} PercentYield=\frac{ActualYield}{TheoreticalYield}*100\% \\ PercentY\imaginaryI eld=\frac{3.80g}{15.7g}*100\operatorname{\%} \\ PercentY\mathrm{i}eld=24.2\% \end{gathered}[/tex]So, the percent yield is 24.2%.
9. Calculate the molarity of a 400.0 mL solution that contains 41.5 g of NaCl.
Answer
1.775 M
Explanation
Given:
Volume of solution, V = 400.0 mL
Mass of NaCl = 45.5 g
What to find:
The molarity of the solution.
Step-by-step solution:
Step 1: Convert the volume from mL to L.
This can be done by dividing the volume in mL by 1000.
V = 400.0 mL = (400.0/1000) = 0.4L
Step 2: Convert the mass of NaCl to moles.
The mass can be converted to moles using the mole formula below:
[tex]\begin{gathered} Moles=\frac{Mass}{Molar\text{ }mass} \\ \end{gathered}[/tex]From the periodic table, the molar mass is determined to be = 58.44 g/mol
Putting mass = 41.5 g and molar mass = 58.44 g/mol into the formula, we have:
[tex]Moles=\frac{41.5g}{58.44g\text{/}mol}=0.7101\text{ }mol[/tex]Step 3: Calculate the molarity of the solution using the molarity formula.
Molarity formula is given by:
[tex]Molarity=\frac{Moles}{Volume\text{ }in\text{ }L}[/tex]Moles= 0.7101 mol and V = 0.4 L
Therefore,
[tex]Molarity=\frac{0.7101mol}{0.4L}=1.775\text{ }M[/tex]The molarity of a 400.0 mL solution that contains 41.5 g of NaCl = 1.775 M.
If compound has molecular weight of 114.22g/mole and its empirical formula is C4H9 FIND its molecular formulaa. C12 H27b) C16 H36c) C8 H18d) C4 H9
Answer
c) C₈H₁₈
Explanation
Given that:
A compound has a molecular weight of 114.22 g/mol
The empirical formula for the compound is C₄H₉
What to find:
To determine the molecular formula for the compound.
Step-by-step solution:
(Empirica formula)n = (Molecular weight)
(C₄H₉)n = 114.22
(4 x 12.01 + 9 x 1.01)n = 114.22
(48.04 + 9.09)n = 114.22
57.13n = 114.22
Divide both sides by 57.13
n = 114.22/57.13
n = 2
Therefore, the molecular formula for the compound is (C₄H₉)₂ = C₈H₁₈
The correct answer is option c) C₈H₁₈
What is the pressure in a 7.00 L tank with 1.73 grams of hydrogen gas at 375 K?
Considering the ideal gas law, the pressure in a 7.00 L tank with 1.73 grams of hydrogen gas at 375 K is 26.5987 atm.
Definition of ideal gas lawAn ideal gas is called a hypothetical or theoretical gas, which would be composed of particles that move randomly and without interacting with each other.
An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar gas constant:
P×V = n×R×T
Pressure in this caseIn this case, you know:
P= ?V= 7 Lmass of hydrogen= 1.73 gmolar mass of hydrogen= 1 g/molen= mass of hydrogen× molar mass of hydrogen= 1.73 g÷ 1 g/mole= 1.73 molesR= 0.082 atmL/molKT= 375 KReplacing in the definition of ideal gas law:
P× 2 L = 1.73 moles ×0.082 atmL/molK ×375 K
Solving:
P= (1.73 moles ×0.082 atmL/molK ×375 K)÷ 2 L
P= 26.5987 atm
Finally, the pressure is 26.5987 atm.
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1. A 26.6g sample of mercury is heated to 110.0℃ and then placed in 125g of water in a coffee-cupcalorimeter. The initial temperature of the water is 23.00℃. (c Hg = 0.139 J/g℃). What is the finaltemperature of the water and the mercury? 2. Draw the Lewis bonding structure for PCl3. what would be the hybrid orbitals
The Lewis structure tells us how atoms are bonded and shows the valence electrons of each element as dots. These valence electrons can be found in the periodic table of the elements, and they coincide with the group number to which the element belongs.
So phosphorus (P) belongs to group 5 and has 5 valence electrons. Chlorine (Cl) is in group 7 and has 7 valence electrons.
The Lewis scheme will be:
The blue dots correspond to the valence electrons of phosphorus, and the purple dots are the electrons of chlorine. The electrons they share can be written with a line.
We have that the geometry of the molecule will be:
Four sp3 type hybrid orbitals are formed, three of which overlap with each of the Cl atoms and the other houses the lone electrons. Sigma type bonds.
Answer: 4 sp3 hybrid orbitals