The flow rate of the IV pump should be 17.06mL/hr.
1st) We need to calculate the patient's weight knowing that 1 lb is equal to 0.45 kg:
[tex]\begin{gathered} 1\text{ lb-0.45 kg} \\ 237\text{ lb - x =}\frac{237\text{ lb}\cdot\text{0.45 kg}}{1\text{ lb}} \\ \\ x=106.65\operatorname{kg} \end{gathered}[/tex]The patient weighs 106.65 kg.
2nd) If the patient needs a drip at 8.0 units per kg of body weight, we have to calculate the units for the patient:
[tex]\begin{gathered} 1\text{ kg - 8.0 units} \\ 106.65\text{ kg - x=}\frac{106.65\text{ kg}\cdot\text{8.0 units}}{1\text{ kg }} \\ \\ x=853.2\text{units} \end{gathered}[/tex]So, the patient needs 853.2 units per hour.
3rd) To calculate the flow rate of the IV pump, we need to know the mL equivalent to 853.2 units:
[tex]\begin{gathered} 25,000\text{ units - 500mL} \\ 853.2\text{ units - x=}\frac{853.2\text{ units}\cdot\text{500mL}}{25,000\text{ units}} \\ \\ x=17.06mL \end{gathered}[/tex]So, the flow rate of the IV pump should be 17.06mL/hr.
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.
What is a molecular equation and how do I do that
option A is is a true molecular equation depicted.
Na2S+2HCl→2NaCl+H2S↑
A molecular equation is a balanced chemical equation in which the constituent ions of the ionic compounds are represented as molecules. Each of a compound's constituent components and the amount of atoms they each possess are listed in the molecular formula. Similar rules apply to the most basic formula: all the constituents are mentioned, but the numbers represent their relative proportions.
There are three different types of equations that may be developed for a reaction involving ionic compounds: molecular equations, full ionic equations, and net ionic equations. In chemistry, each of these equations has a specific function. Because it details exactly which compounds were employed in a process, a molecular equation is useful.
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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
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
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
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.
Why is DNA describes as a blueprint for a cell?
DNA describes as a blueprint for a cell because it contain the instruction needed for an organism to grow develop and survive
DNA is called a blueprint of life because it contain the instruction needed for an organism to grow develop and survive and reproduce and DNA does this by controlling protein synthesis and protein do must of the work cell and are basic unit of structure and function in the cell of organism
DNA is read by the enzyme RNA polymerase and this enzyme attaches itself to the DNA strand slightly in front of a gene and it then slides along the DNA strand making a copy of the gene only using RNA building blocks instead of DNA building block
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Radioactive iodine (I-131) is an isotope of iodine that emits radiation and is used for various medical applications, such as in the treatment of thyroid cancer. The half-life for I-131 is 8 days. Based on the half-life of I-131, how many half-lives have to pass for a 200 mg sample of I-131 to decay down to 25 mg?
Half life is the time period in which half of the initial amount of an element will decay into a new element due to instability. For I-131, the half life is 8 days.
From 200 to 25 grams, let's see how many half lives are there:
200g -> 100g
100g -> 50g
50g -> 25g
Therefore for 200g of I-131 reach 25 grams, 3 half lives are necesseray, 3 half lives or 24 days
could you calculate the percent composition for 15 and the empirical formal for 16
To solve this question, we need to know the molar mass of Ca. It is 40 g/mol
There are 3 atoms of Ca in Ca3(PO4)2
So the mass of Ca in Ca3(PO4)2 is 3x40 = 120 g
So:
375 grams ---- 100%
120 g --- x
x = 32%
Answer: 32% of calcium.
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 is the % concentration by mass of 3.5 g of NaCl dissolved in 100.0 grams of water
Step 1 - Understanding % concentration in mass
% concentration in mass expresses the concentration of a solute by its percentage, in mass, in relation to the total mass of the solution.
Mathematically, we can find this percentage by the following relation:
[tex]\text{ \%concentration = }\frac{m_{solute}}{m_{solution}}\times100[/tex]Step 2 - Caculating the % concentration for the given solution
According to the exercise:
[tex]\begin{gathered} m_{solute}=3.5g\text{ \lparen NaCl is the solute\rparen} \\ \\ m_{solution}=100+3.5=103.5 \end{gathered}[/tex]Setting these values in the equation:
[tex]\text{ \%concentration = }\frac{3.5}{103.5}\times100=3.38\text{ \%}[/tex]Answer: the % concentration of NaCl in this solution is 3.38%.
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
Calculate the pOH for an aqueous solution containing 0.01 moles of HCl in a 2.5 L solution.
The question requires us to calculate the pOH value for a solution containing 0.01 moles of HCl in 2.5 L of solution.
To solve this problem, we'll need to go through the following steps:
I) calculate the molar concentration of the HCl solution to obtaine the concentration of H+ ions;
II) using the concentration of H+ ions, calculate the pH of the solution;
III) with the value obtained for pH, calculate the value of pOH for this solution.
Next, we'll go through the steps to solve the question:
I) Since the question provided the number of moles of HCl and the volume of the solution, we can calculate the molar concentration using the following equation:
[tex]\text{molar concentration = }\frac{\text{number of moles (mol)}}{\text{volume (L)}}_{}[/tex]Thus, applying the values provided:
[tex]\text{molar concentration of HCl= }\frac{0.01\text{ mol}}{2.5\text{ L}}=0.004\text{ mol/L}[/tex]Therefore, the concentration of the HCl solution is 0.004 mol/L.
Since HCl is a strong acid, we can expect it to completely dissociate in H+ and Cl-: the concentration of H+ ions for this solution would also be 0.004 mol/L ( [H+] = 0.004 mol/L).
III) The next step is calculate the pH of this solution. We'll use the following equation and apply the concentration of H+ ions obtained in the previous step ( [) using H+] = 0.004 mol/L):
[tex]pH=-\log _{10}\lbrack H^+\rbrack\to pH=-\log _{10}(0.004)=2.39[/tex]Now, we know that the pH of the solution is 2.39.
III) The last step is use the pH value calculated (pH = 2.39) to calculate the pOH of the solution, using the following equation:
[tex]pH+\text{pOH =14}\to pOH\text{ = 14 - pH}[/tex][tex]\text{pOH = 14-2.39 = 11.6}[/tex]Therefore, the pOH of the HCl solution given is 11.6.
Calculate ∆G° for each reaction using ∆Gf° values: (a) 2Mg(s) + O2(g) → 2MgO(s)
The free energy of formation of the MgO is −597 kJ/mol.
What is the standard free energy of formation?We know that the free energy of formation is defined as the energy that is evolved or absorbed when a substance is formed from its components under standard conditions. In this case, we have that the magnesium and the oxygen are all pure substances.
It is important that we recall that the free energy of formation of a pure substance is zero. We have the free energy of formation of the magnesium oxide as−597 kJ/mol.
Hence;
Sum of free energy of formation of products - Sum of free energy of formation of reactants
We have;
(−597 kJ/mol) - (0 kJ/mol)
free energy of formation = −597 kJ/mol
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What is the pH of a Strong Acid solution whose concentration is 10-7M?
Answer
pH = 6
Explanation
Given that:
The concentration of the acid [H⁺] = 10⁻⁷ M
What to find:
The pH of the strong acid solution.
Step-by-step solution:
The pH of the strong acid solution whose concentration is 10⁻⁷ M can be calculated using the pH formula.
The pH formula is given by: pH = -log[H⁺]
Substitute [H⁺] as 10⁻⁷ M, we have:
pH = - log(10⁻⁷)
pH = -(-6)
pH = 6
The pH of the strong acid solution whose concentration is 10⁻⁷ M is 6.
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
pls help meHow many liters of NH3 are needed to react completely with 30.0 L of NO (at STP)?4NH3 (g)+ 6NO(g) 5N2(g)+ 6H2o(g)a.5.0 Lc.7.5 Lb.20.0 Ld.120.0 L
Answer:
[tex]20.0\text{ L}[/tex]Explanation:
Here, we want to get the volume of NH3 that will react with 30L of NO at STP
From the question, we have it that 4 moles of ammonia reacted 6 moles of NO
Thus, we have the mole ratio as 6 to 4
Thus, the volume of ammonia reacted would be:
[tex]\frac{4}{6}\times30\text{ = 20.0 L}[/tex]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
Please help with 2nd and 3rd questions In question b) Aluminum reacts with hydrocloric acid
In order to solve the question b):
We have the following reaction occuring:
[tex]2Al+6HCl\rightarrow2AlCl_3+3H_2[/tex]We need to calculate the number of moles of aluminum needed to produce 30ml of H2 (hydrogen gas) at a temperature of 22°C and a pressure of 763mmHg.
To calculate the number of moles of hydrogen produced we use the ideal gas equation:
[tex]P.V=n.R.T[/tex]Where:
P is the pressure
V is the volume
n is the number of moles
R is the gas constant
T is the temperature
R is a constant and it's value is:
[tex]R=8.314\text{ }\frac{m^3.Pa}{K.mol}[/tex]So we need to convert each variable to the units of this constant.
[tex]\begin{gathered} T:\text{ }22^{\circ}C=295.15^{\circ}K \\ P:\text{ }763mmHg=101725\text{ }Pa \\ V:\text{ 30ml}:0.00003m^3 \end{gathered}[/tex]So now we calculate:
[tex]n=\frac{P.V}{R.T}=\frac{101725Pa.0.00003m^3}{8.314\frac{m^3.Pa}{K.mol}.295.15^{\circ}C}=0.00124mol[/tex]So we know that 0.00124 moles of H2 are formed.
Now we know that for every 2 moles of aluminum 3 moles of H2 are formed.
So we calculate the moles of Al needed:
[tex]n_{Al}=0.00124mol_{H2}.\frac{2mol_{Al}}{3mol_{H2}}=0.000826mol_{Al}[/tex]So the answer is 0.000826 moles of Al°
Balance the following chemical equation using algebraic method ( A value is 2 ) ( please include procedure ) Sn (NO2)4 + Pt3N4 = Sn3N4 + Pt(NO2)4
Given the equation:
• Sn (NO2)4 + Pt3N4 → Sn3N4 + Pt(NO2)4
(1) The first thing we noticed is that this is a double replacement equation
• ,Sn combines with N4 to form Sn3N4, (,take note that Sn→ Sn3,)
• Pt3 combines with (NO2) to form Pt(NO2)4 ( ,take note that Pt3 → Pt)
(2) Balancing the equation
• Sn (NO2)4 + Pt3N4 → Sn3N4 + Pt(NO2)4 ....(,place 3 infront of Sn in the reactant side .)
• 3,Sn (NO2)4 + Pt3N4 → Sn3N4 + Pt(NO2)4...( ,then place 3 infront of Pt in the product side,)
,• 3,Sn (NO2)4 + Pt3N4 → Sn3N4 + ,3,Pt(NO2)4
Check :
3Sn reactant : Sn3 Product
(NO2)4 reactant : (NO2)4 product
Pt3 reactant : 3Pt product
N4 reactant : N4 product
RHS = LHS ,this means that our equation has now balance.% w/v relates which two units?A.grams and molesB.grams and millilitersC.moles and litersD.temperature and volumeE.milliliters and moles
Explanation:
The % w/v s the number of grams of solute in 100 mL of solution
So it relates grams of solute with mL of solution.
Answer: B. grams and milliliters
2. Complete and correctly balance each of the following reactions: 5 pts(a) Double replacement: Ba Cl2 (aq) + AgNO3 (aq)-(b) Decomposition: HgO (s)(c) Combustion: C4H10 (9) + O2 (9)-(d) Single replacement: Ca (s) + AlCl3 (s)(e) Combination: Mg(s) + N2 (9)-
2. (a) We are told that it is a double displacement reaction, so there will be two substitutions and Cl will exchange places with NO3.
Now, that will be the full reaction but we need to balance it. Count the atoms of each element on each side of the reaction. In the figure we can see that Chlorine, Nitrogen and Oxygen are not balanced.
We place the coefficient 2 in front of the AgCl molecule to balance the chlorides. You can see the picture.
Now we will balance the nitrogens. There are two nitrogens in the products. We place the coefficient two in the AgNO3 molecule. In the figure I will make the update.
Now the equation is balanced, so the balanced reaction will be:
[tex]BaCl_{2(aq)}+2AgNO_{3\left(aq\right)}+\rightarrow Ba\left(NO_3\right)_{2\left(aq\right)}+2AgCl(s)[/tex]How many grams of glucose are required to heat 175 mL of water from 20.0 °C to 25.0°C?
We must first determine the heat needed to heat 175mL of water. In the working temperature range we can assume that the density of water is 1g/mL, so the mass of water that we must heat will be 175g of water.
Now, the heat we need to heat that mass of water is calculated with the following equation:
[tex]Q=mCp\Delta T[/tex]Where Q is the heat required to heat the water
Cp is the specific heat of water equal to 4186 J/g°C
delta T is the change of temperature = 25°C-20°C=5°C
We replace the know values:
[tex]Q=175g\times4186\frac{J}{g\degree C}\times\frac{1kJ}{1000J}\times5\degree C=3662.75kJ[/tex]Now, to heat the water they tell us that the glucose combustion will take place. We must assume that all the heat generated in the reaction will go to heating the water and that there is no heat loss to the environment.
The combustion reaction of glucose generates 2538.7 kJ/mol. So the moles of glucose needed will be:
[tex]\begin{gathered} molGlucose=givenHeatrequired\times\frac{1molGlucose}{2538.7kJ} \\ molGlucose=3662.75kJ\times\frac{1molGlucose}{2,538.7kJ}=1.44molGlucose \end{gathered}[/tex]We calculate the grams of glucose by multiplying the moles by the molar mass of glucose equal to 180.2g/mol
grams of glucose= 1.44 mol x 180.2 g/mol=260g
Answer: To heat 175 mL of water from 20.0 °C to 25.0°C are required 260g of glucose
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]A sample of helium gas initially at 0.90 atm is cooled from 18 degreeC to -48 degreeC at constant volume. What is the final pressure?
Answer: By using Ideal gas law PV=nRT ,the final pressure is calculated
Explanation:
In thermodynamics a constant volume process is known as isochoric process and in this volume remains constant and pressure varies along with the temperature .
FORMULA USED - PV=nRT
If Volume is constant ,then initial Temperature = 18+273 = 291K
final temperature =225K
initial pressure = 0.90 atm
final pressure = ?
The final pressure comes out to be 0.6958 atm.
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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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Finish balancing:__al + 3zn(no3)2 -> __al(no3)3 +__znWhat coefficient does al(no3)3 have in the balanced equation?
In order to properly balance an equation, we need to make sure that the same amount of elements on the reactants side matches the number of elements on the products side, we can do that by increasing the number in front of each molecule, the so called stoichiometric coefficient. In the reaction from the question we can properly balance by adding the following stoichiometric coefficients
For our question, we have:
2 Al + 3 Zn(NO3)3 -> 2 Al(NO3)3 + 3 Zn
Now this reaction is properly balanced
Al(NO3)3 has the coefficient 2
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
Do neutrons have postive,negative, or neutral charge ?
Answer:
Balls uhhh neutron but if theres a better answer take it cuz im prolly wrong
Explanation:
50/50 im right up to you to take the chance or jus search it on tha goog
Which types of electron orbitals will have higher energy than a 4d orbital?A. 4pB. 3sC. 4fD. 5s
5s. Option D is correct
Explanations:What are electron orbitals?Electron orbitals are area around the nucleus where electron resides. The closer the orbital to the nucleus, the higher the energy level.
Based on the explanation above, 5s will be higher in energy than the 4d orbital.