What is the value of the smallest bond angle in icl4−? enter the smallest bond angle of the molecule?

Answer:

The theoretical yield is calculated from the amount of the limiting reactant present.

Explanation:

The limiting reactant is one which is present in lesser amount than the other reactant (based on molar ratio requirement)

For example in formation of water we need one mole of hydrogen gas and half moles of oxygen gas. Now we have one mole of hydrogen gas and one mole of oxygen gas then the limiting reagent is hydrogen gas.

theoretical yield is the expected yield of a reaction calculated based on the moles or amount of limiting reagent present as the limiting reagent is going to be completely consumed during the reaction.

Answer : The correct option is, (D) The theoretical yield is calculated from the amount of the limiting reactant present.

Explanation :

Excess reagent : It is defined as the reactants not completely used up in the reaction.

Limiting reagent : It is defined as the reactants completely used up in the reaction.

Theoretical yield : It is calculated from the amount of the limiting reagent present in the reaction.

Actual yield : It is experimentally determined.

Hence, the correct option is, (D) The theoretical yield is calculated from the amount of the limiting reactant present.

The average atomic mass of an element on the periodic table is a weighted average and not a whole number because it accounts for the different masses and abundances of each isotope, whereas the actual mass of an individual atom is approximately its mass number, a whole number.

You will never find an atom that has an actual atomic mass equal to the average atomic mass of the element because the atomic mass listed on the periodic table is a weighted average of all the naturally occurring isotopes of that element. Because each proton and each neutron has a mass of approximately one atomic mass unit (amu), and electrons contribute much less, the atomic mass of each isotope is approximately equal to its mass number, which is always a whole number. However, the average atomic mass is not a whole number because it is a calculation that includes the different masses of each isotope and their respective abundance percentages. This weighted average reflects the average mass of an atom if you could randomly pick one out of a sample containing all the isotopes of that element.

For example, carbon has two stable isotopes, 12C and 13C, with respective abundances of 98.89% and 1.11%. The average atomic mass of carbon is calculated by taking into account these abundances, leading to an average atomic mass that does not match exactly the mass of either isotope. In contrast, some elements have atomic masses in square brackets, like technetium (element 43) and promethium (element 61), which indicate the mass number of their most stable isotope because these elements do not have stable isotopes with an average atomic mass.

Answer : The correct option is, [tex]1.63\times 10^{-3}g[/tex]

Explanation : Given,

Mass of oxygen gas = [tex]1.45\times 10^{-3}g[/tex]

Molar mass of oxygen gas = 32 g/mole

Molar mass of water = 18.02 g/mole

First we have to calculate the moles of [tex]O_2[/tex].

[tex]\text{Moles of }O_2=\frac{\text{Mass of }O_2}{\text{Molar mass of }O_2}=\frac{1.45\times 10^{-3}g}{32g/mole}=4.53\times 10^{-5}moles[/tex]

Now we have to calculate the moles of [tex]H_2O[/tex].

The balanced chemical reaction is,

[tex]2H_2+O_2\rightarrow 2H_2O[/tex]

From the balanced reaction we conclude that

As, 1 mole of [tex]O_2[/tex] react to give 2 mole of [tex]H_2O[/tex]

So, [tex]4.53\times 10^{-5}[/tex]moles of [tex]O_2[/tex] react to give [tex]4.53\times 10^{-5}\times 2=9.06\times 10^{-5}[/tex] moles of [tex]H_2O[/tex]

Now we have to calculate the mass of [tex]H_2O[/tex]

[tex]\text{Mass of }H_2O=\text{Moles of }H_2O\times \text{Molar mass of }H_2O[/tex]

[tex]\text{Mass of }H_2O=(9.06\times 10^{-5}mole)\times (18.02g/mole)=1.63\times 10^{-3}g[/tex]

Therefore, the mass water produced is, [tex]1.63\times 10^{-3}g[/tex]

Copper, silver, mercury, and gold are less reactive than hydrogen as they are positioned at the bottom of the activity series and do not readily react with acids to produce hydrogen gas.

The metals listed that are less reactive than hydrogen (H2) are those found at the bottom of the activity series. Specifically, these metals include copper (Cu), silver (Ag), mercury (Hg), and gold (Au). These metals do not react with acids to form hydrogen gas and hence are considered less reactive than hydrogen. Additionally, in the context of the electrochemical series, these metals are known as inert metals, indicating their low reactivity and their position at the very bottom of the activity series. Therefore, they do not readily corrode in the presence of dilute acids.

It's important to note that aside from basic trends, the exact order of reactivity of metals can be determined from the activity series or electrochemical series, where the lower a metal's position relative to hydrogen, the less reactive it is in comparison.

The wavelength (in nanometers) of a photon emitted by a hydrogen atom when its electron drops from the n = 5 to n = 3 state is 1280nm.

The term wavelength defined as the distance between the two successive crests or troughs of the wave. Wavelength is denoted by the greek word lambda (λ).

The distance between the "crest"  of one wave to the crest of the another wave is the wavelength. We can measure from the "trough" of one wave to the trough of the another wave we get the same value for the wavelength.

The difference in energy (E) between two shells calculated as follows:

ΔE = -RH [(1 / nf2) - (1/ni2)] ΔE

= -2.18 x10-18 J [(1/32) - (1/52)] ΔE

= -1.55 x10-19 JE

hc/λλ = hc/Eλ

= [(6.63 x10-34 J.s.) x (3.00 x1017 nm/s)] /(1.55 x10-19 J)

λ = 1280nm

Thus, The wavelength of a photon emitted by a hydrogen atom when its electron drops from the n = 5 to n = 3 state is 1280nm.

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The student's question involves predicting the formulas of new combinations of elements to form binary ionic compounds. The correct formulas are based on the charges of the ions, aiming for a neutral overall charge. Examples include KCl for potassium + chlorine, AlF3 for aluminum + fluorine, and SnO2 for tin + oxygen.

The student is asking for the predicted formulas of new chemical combinations by replacing elements in known compounds utilizing the rules for writing formulas of binary ionic compounds. The key to solving this problem is to balance the charges of the ions so that the overall charge of the compound is neutral. When predicting the formulas, we need to consider the valency or oxidation states of the elements involved. For example, if potassium (K) replaces sodium (Na) in sodium chloride (NaCl), since both have a +1 charge, the new formula would be KCl. Following a similar process, substituting aluminum (Al) for aluminum in aluminum fluoride (AlCl3) with fluorine (F), considering aluminum has a +3 charge and fluorine has a -1 charge, results in the formula AlF3. The charge of tin (Sn) is +2 or +4, but when combined with oxygen (O), which has a -2 charge, a likely compound could be SnO2, assuming tin is in the +4 oxidation state.

Let's predict the remaining chemical formulas based on the initial list:

Its dune. The Delta landform is involving water, not sand. Dunes are basically sand, so i would pick dune

Final answer:

To determine the number of moles of nitrogen in 1.61 x 10²⁴ nitrogen particles, divide by Avogadro's number, resulting in 2.673 moles of nitrogen.

Explanation:

The student is asking about the number of moles of nitrogen contained in a given number of nitrogen particles. To find this, we use Avogadro's number, which is the number of particles in one mole of a substance. The value of Avogadro's number is 6.022 x 10²³ mol−1. Since the question indicates that there are 1.61 x 10²⁴ nitrogen particles, we divide this number by Avogadro's number to determine the moles.
Here's the calculation:
Number of moles (n) = Number of particles (N) / Avogadro's number (NA)
n = 1.61 x 10²⁴ particles / 6.022 x 10²³ mol−1
n = 2.673 moles of nitrogen

Copper has an atomic number of 29, 4 copper atoms contain 116 electrons, while 3 copper atoms can be formed from 87 protons.

The atomic number of an element tells us the number of protons in an atom of that element.

1. Since copper has an atomic number of 29, each copper atom has 29 electrons as well. To find the total number of electrons in 4 atoms of copper, we can simply multiply the number of electrons in one copper atom by 4.

So, there are 4 [tex]\times[/tex] 29 = 116 electrons in 4 atoms of copper.

2. Since each copper atom has 29 protons, we can divide the total number of protons by 29 to find the number of copper atoms that can be made.

[tex]\dfrac{87}{29} = 3[/tex]

So,87 protons can make 3 copper atoms.

Therefore, there are 116 electrons in 4 atoms of copper and 3 copper atoms can be made out of 87 protons, respectively.

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Aluminum sulfide is Al₂S₃, which shows that there are 3 sulfur atoms per formula unit.

In one mole there is Avogadro’s number of atoms and Avogadro’s number = 6.02 x 10²³

In 1.10 mole = 1.10 x 6.02x10²³ = 6.62 x 10²³ formula units

Now multiply with 3 to get number of sulfur atoms present in 1.10 mol of Aluminum sulfide;

3 x 6.62x10²³ = 1.99 x 10²⁴

So, the answer is 1.99 x 10²⁴ sulfur atoms.

The electrons in the higher energy level of an atom which determines the chemical properties of the atom and involved in chemical bonding are called the valence electrons.

An atom is composed of electrons, protons and neutrons. Protons and neutrons are located inside inside the core of atom called nucleus. Electrons are revolving around around the nucleus through circular paths of definite energy.

The regions where the electrons can be seen is called orbital. The electrons in the orbitals closer to the nucleus is called the core or inner electrons. The electrons which are in the outer shells away from the nucleus is called valence electrons.

Valence electrons are free to interact with the surrounding environment and they are participating in chemical bonding to form compounds. When the valence shells attain octet, they are said to be stable. Therefore, the atoms with electron deficient or extra electrons in the valence shell bonds with other atoms.

Therefore, the number of valence electrons determines the chemical properties of the atom.

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Answer:

it is c

Explanation:

The solution is not a pure substance because it is a mixture between a solute and a solvent. Therefore, option (C) is correct.

Pure substances can be described as elements that cannot be broken down into simple substances that contain only one kind of atom in the whole composition.

A pure substance can be described as made up of two or more chemical elements that are chemically combined and has a set composition such type of pure substance is called a compound. For example, water is a pure compound that is composed of hydrogen and oxygen in a whole ratio of 2:1.

A mixture can be described as made up of two or more different substances which are only physically combined but not chemically. A mixture can be separated into its original components.

The composition of a heterogeneous mixture does not have uniform throughout the mixture while the composition in a homogeneous mixture is always the same.

Therefore, the solution is a mixture, not a pure substance.

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The particle that an atom can lose or gain in order to form a charged ion is electron.

When an atom lose an electron from their valence shell the it form positive charged ion known as cation.

When an atom gain an electron from their valence shell then it form negative charged ion known as anion.

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Answer:

1. less reactive than sodium

Explanation:

Isotopes of a particular element are alike in that they all have the same atomic number which means they have the same number of protons. However, they differ in the number of neutrons.

The isotopes of a particular element are alike in that they all have the same number of protons in the nucleus, hence, they are all part of the same atomic family and share the same atomic number. This determines the element's position in the periodic table and its chemical properties. For example, all isotopes of Hydrogen - Protium, Deuterium and Tritium - have one proton each.

However, isotopes of a same element differ in their number of neutrons. For instance, while Protium has no neutrons, Deuterium has one and Tritium has two.

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Uv gel enhancements rely on ingredients from the monomer liquid and acrylic chemical family.