How reactive is an atom of Sodium(Na) and why?




Question 1 options:


Sodium (Na) is very reactive because it does not have a full valence shell.



Sodium (Na) is very reactive because it does not have enough protons in the nucleus.



Sodium (Na) is not very reactive because it does not have a full valence shell.



Sodium (Na) is not very reactive because it can only bond with Chlorine (Cl) to become salt.


PLz plz plz plz help

The chemical reaction that requires 31.39 kilojoules equate to approximately 7.5 kilocalories, as 1 kilocalorie equals approximately 4.184 kilojoules.

To convert kilojoules to kilocalories, you need to use the conversion factor of 1 kilocalorie equals approximately 4.184 kilojoules. Therefore, to find the equivalent in kilocalories for 31.39 kilojoules, you divide 31.39 by 4.184.

So, the calculation will be 31.39 kJ / 4.184 kcal/kJ = ~7.5 kcal. Hence, the chemical reaction that requires 31.39 kj is equivalent to about 7.5 kilocalories.

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When a non-metal atom becomes an anion, the addition of electrons increases electron-electron repulsion, causing the size of the atom to increase. Option B. it increases is correct option.

When a non-metal atom becomes an anion, it gains one or more electrons. Since electrons are negatively charged and repel each other, adding more electrons causes an increase in electron-electron repulsion. This increased repulsion causes the electron cloud to expand, resulting in the size of the atom increasing.

The correct answer is B. it increases.

To calculate this,

We know that energy is 1 photon 
E = hc/wavelenth 
wavelength of 10.0 m 

Solution:
h = 6.626 x 10^-34 Jsec 
C = 2.9979 x 10^8 m/sec 
E = 6.626 10^-34 * 2.9979 10^8 / 10 = 1.9864 10^-26J 

Then, the number of photons is computed by:

n = 1000 / 1.9864 10^-26 = 5.04 10^28 photons 

The empirical formula of the compound is CH5O after dividing the molar amounts of carbon, hydrogen, and oxygen by the smallest molar amount and adjusting to get whole numbers.

To calculate the empirical formula of the compound, we first need to find the molar amounts of each element based on their given masses. For carbon (C), we divide 330 g by its molar mass of 12.01 g/mol, which gives us 27.48 mol. For hydrogen (H), 69.5 g divided by 1.008 g/mol gives us 68.95 mol. For oxygen (O), 440.4 g divided by 16.00 g/mol gives us 27.53 mol. Next, we divide each molar amount by the smallest molar amount to get the simplest whole number ratio.

The smallest molar amount is 27.48 mol (for carbon), so we divide each element's molar amount by 27.48 mol. The resulting ratios are 1 for carbon, approximately 2.51 for hydrogen, and 1 for oxygen. The closest whole number ratio would then be interpreted as a 1:2.51:1 ratio, which we can approximate as 1:2.5:1. To convert it into whole numbers, we can multiply all the numbers by 2 to get the empirical formula C1H5O1, or simply CH5O.

Final answer:

By calculating the number of moles of carbon, hydrogen, and oxygen from the given masses and finding their simplest whole number ratio, the empirical formula of the compound is determined to be C₂H₅O₂.

Explanation:

Calculating the Empirical Formula:

To find the empirical formula of the compound, we need to convert the given masses of carbon (C), hydrogen (H), and oxygen (O) to moles. This is done by dividing the mass of each element by its respective atomic weight. The atomic weights of C, H, and O are 12.01 g/mol, 1.008 g/mol, and 16.00 g/mol, respectively. Hence, the number of moles of each element can be calculated as follows:

Next, we determine the simplest whole number ratio of the moles of each element by dividing each value by the smallest number of moles calculated:

To convert these ratios to whole numbers, we can multiply each ratio by a common factor that converts the smallest decimal (in this case, the ratio of hydrogen) into a whole number, which is approximately 2 in this case. This gives us whole number ratios of:

Therefore, the empirical formula of the compound is C₂H₅O₂ .

Molecular formula of Isoflurane is C₃H₂ClF₅O.

Now calculate the percent composition by mass, which means percent of each element in the compound.

Mass of Isoflurane = 184.49 g/mol

Mass of carbon in the compound = 3 x 12.011 = 36.033g

Mass of hydrogen in the compound = 2 x 1.008 = 2.016g

Mass of chlorine in the compound = 1 x 35.453 = 35.453 g

Mass of fluorine in the compound = 5 x 18.998 = 94.99g

Mass of Oxygen in the compound = 1 x 16 = 16 g

Carbon’s percentage = Mass of carbon in the compound /mass of isoflurane x 100 =36.033/184.49 x 100 =19.53%

Hydrogen’s Percentage = Mass of hydrogen in the compound/mass of isoflurane x 100 = 2.016/184.49 = 1.09%

Chlorine’s percentage = Mass of chlorine in the compound/mass of isoflurane x 100 = 35.453/184.49 =19.22%

Flourine’s percentage = Mass of fluorine in the compound/mass of isoflurane x 100 = 94.99/184.49 x 100 = 51.49%

Oxygen’s percentage = Mass of Oxygen in the compound/mass of isoflurane x 100 =16/184.49 x 100 = 8.67%

The molecular formula of isoflurane is C3H2ClF5O. The percent composition by mass is approximately: C: 19.54%, H: 1.04%, Cl: 19.25%, F: 51.93%, O: 8.23%.

The molecular formula for isoflurane is C3H2ClF5O. To calculate its percent composition by mass, we need to determine the molar mass of isoflurane and then find the contribution of each element to the total mass.

The molar mass of isoflurane can be calculated by summing the atomic masses of each element in the formula:

Molar Mass = (3 x Atomic Mass of C) + (2 x Atomic Mass of H) + Atomic Mass of Cl + (5 x Atomic Mass of F) + Atomic Mass of O

Using the atomic masses from the periodic table, we can calculate:

Molar Mass = (3 x 12.01) + (2 x 1.01) + 35.45 + (5 x 18.99) + 16.00

Molar Mass = 184.06 g/mol

Calculating Percent Composition

The percent composition by mass of an element in a compound is given by:

Percent Composition = (Mass of Element / Total Mass of Compound) x 100

We can calculate the percent composition for each element in isoflurane by dividing the mass contribution of the element by the total molar mass:

% C = (3 x Atomic Mass of C) / Molar Mass x 100

% H = (2 x Atomic Mass of H) / Molar Mass x 100

% Cl = Atomic Mass of Cl / Molar Mass x 100

% F = (5 x Atomic Mass of F) / Molar Mass x 100

% O = Atomic Mass of O / Molar Mass x 100

Substituting the atomic masses and molar mass values, we can calculate the percent composition:

% C = (3 x 12.01) / 184.06 x 100 = 19.54%

% H = (2 x 1.01) / 184.06 x 100 = 1.04%

% Cl = 35.45 / 184.06 x 100 = 19.25%

% F = (5 x 18.99) / 184.06 x 100 = 51.93%

% O = 16.00 / 184.06 x 100 = 8.23%

So, the percent composition by mass of isoflurane is approximately:

Explanation:

A mixture in which all the solute particles distribute uniformly into the solvent is known as a homogeneous mixture.

A homogeneous mixture is a clear solution with no solute particles seen in it.

For example, isopropyl alcohol is a clear solution. Hence, it is a homogeneous mixture.

On the other hand, a heterogeneous mixture is defined as the mixture in which solute particles are not uniformly distributed into the solvent.

For example, sand dissolved in water is a heterogeneous mixture.

Thus, we can conclude that isopropyl alcohol is a homogeneous mixture.

Isopropyl alcohol, also known as rubbing alcohol, is considered a homogeneous mixture.

A homogeneous mixture is a uniform mixture with the same composition and properties throughout. In the case of isopropyl alcohol, it consists of molecules of isopropyl alcohol uniformly distributed in the solvent (usually water).

It does not separate into distinct phases and exhibits the same characteristics and properties regardless of the location within the mixture.

Learn more about isopropyl alcohol at

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First let us calculate the number of moles.

number of moles = (5.0 x 10^-25 g) / (26.98154 g/mol)

number of moles = 1.853 x 10^-26 mol

We then calculate the number of atoms using Avogadros number.

number of atoms = (1.853 x 10^-26 mol) * (6.022 x 10^23 atoms / mole)

number of atoms = 0.011 atoms

There can never be an atom of less than 1 since 1 unit of atoms is the basic unit of all elements. Therefore it is NOT possible.

Final answer:

While the atomic mass of Aluminum is 26.98 g/mol, indicating one mole of Aluminum atoms weighs 26.98 g, the asked mass of 5.0 x 10^-25 g is far lower, representing a fraction of a single atom of Aluminum. Considering atoms cannot physically be divided into smaller portions without ceasing to be that element, it is not possible to have 5.0 x 10^-25 g of Aluminum.

Explanation:

The question asks if it is possible to have 5.0 x 10^-25 g of Aluminum (Al), given that the atomic mass of Al is 26.98154 g/mol. To answer this, one must understand the concept of Atomic Mass and Molar Mass.

The atomic mass of Al is approximately 26.98 g/mol, which means one mole of Al atoms has a mass of 26.98 g. However, the mass in question (5.0 x 10^-25 g) is significantly smaller than this.

Considering that the mass of a single atom of Al is on the order of 10^-23 g (since 1 mol of Al has a mass of 26.98 g and includes Avogadro's number of atoms, approximately 6.02 × 10^23), having a mass of 5.0 x 10^-25 g of Al would represent a fraction of an Al atom, which is not physically possible.

This is because atoms are the smallest unit of matter that retains the properties of an element, and they cannot be divided into smaller units without losing the properties that define them as that element.

The chemical reaction for this is in the form of:

Na + Cl + O --> NaClO

The elements on the left side of the --> symbol are the reactants while on the right side we can find the product. Therefore the reactants are:

Na, Cl, and O

The chemical reaction for this is in the form of:

Na + Cl + O = NaClO

To produce 8g of silver, you'd need approximately 4.7g of copper, assuming a 1:1 molar ratio in their reaction.

Before calculating the grams of copper needed to produce 8 grams of silver, you first need to express the mass of silver in moles. To do this, divide the mass by the atomic mass of silver. Next, find the molecular ratio in the reaction of copper to silver. In this case, we'll treat it as a 1:1 ratio as the question didn't provide one. Hence, the moles of copper required will be the same we calculated for silver. Lastly, convert these moles of copper back into grams using the atomic mass of copper.

Let's put this into practice:

So, you will need approximately 4.7 g of copper to produce 8 g of silver, given a 1:1 molar ratio in their reaction.

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Great conductor of heat and electricity: Barium

Malleable and highly reactive: Potassium

Has properties of both metals and nonmetals: Boron

Nonreactive gas: Neon

For more information about the elements of the periodic table, refer to the link:

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Potassium is a metal that is a great conductor of heat and electricity. Barium is a highly reactive metal. Boron is a metalloid with properties of both metals and nonmetals. Neon is a nonreactive gas.

Potassium is a great conductor of heat and electricity, making it a metal. Barium is an element that is shiny, malleable, and highly reactive, also a metal. Boron is a metalloid, which means it has properties of both metals and nonmetals. Neon is a nonreactive gas.

Potassium is best matched with 'Malleable and highly reactive', Barium with 'Great conductor of heat and electricity', Boron with 'Has properties of both metals and nonmetals', and Neon with 'Nonreactive gas'.

The solution for this problem would be:

We are looking for the grams of magnesium that would have been used in the reaction if one gram of silver were created. The computation would be:

1 g Ag (1 mol Mg) (24.31 g/mol) / (2mol Ag)(107.87g/mol) = 0.1127 grams of Magnesium

Final answer:

To calculate the grams of magnesium needed to produce 1.000 g of silver, we use the stoichiometry of the reaction and the molar masses of magnesium and silver. The result is 0.1128 grams of magnesium.

Explanation:

To determine how many grams of magnesium would have been used in the reaction if 1.000 g of silver were produced, we first need to understand the stoichiometry of the reaction. Assuming magnesium reacts in the same way as copper, let's consider a simple replacement reaction where magnesium would replace silver in a compound:

Mg + 2 AgNO3 → Mg(NO3)2 + 2 Ag

The atomic ratio and stoichiometry suggest that for every mole of magnesium, two moles of silver are produced. Since the atomic mass of silver (Ag) is 107.87 g/mol, the molar mass of magnesium (Mg) is 24.31 g/mol, and we have produced 1.000 g of Ag, we can perform the following calculations:

Calculate moles of Ag produced: (1.000 g Ag) / (107.87 g/mol) = 0.00928 moles of Ag.

Given the stoichiometry of the reaction, 1 mole of Mg produces 2 moles of Ag. Therefore, for 0.00928 moles of Ag, half the amount of Mg would react, which is 0.00928 / 2 = 0.00464 moles of Mg.

To find the grams of Mg: (0.00464 moles Mg) × (24.31 g/mol) = 0.1128 grams of Mg.

So, 0.1128 grams of magnesium would have been used to produce 1.000 g of silver.

Answer:

C) Newton's discoveries of the laws of motion.

Explanation:

Basic research is based on understanding of the natural phenomena. Like understanding why the apple fell down from a tree instead of going up in the sky. This thought propelled Newton to discover the laws of gravitation. Applied research on the other hand is about the discovery of technology that can harness the natural resources. Such as the discovery of solar panels and wind mills etc.

Answer: Option (a) is the correct answer.

Explanation:

When there occurs no change in chemical composition of a substance then it is known as a physical property.

For example, volume, mass, shape, size, density etc are all physical properties.

In liquids, the molecules are held by slightly less strong intermolecular forces of attraction as compared to a solid. So, the molecules of a liquid are able to slide over each other as they have kinetic energy.

Therefore, a liquid has indefinite shape because they acquire the shape of container in which they are placed. But a liquid does not have a definite volume.

Thus, we can conclude that indefinite volume is not a physical property of a liquid.

We start with an initial pH and transform this into moles. We then add a specified amount of HCL and calculate the new amount of moles. Then we calculate the remaining concentration of the acid by taking the difference of the initial and the added amounts. We convert volumes for values into required units for the proper calculation of the final concentration of HCl.

To find the additional volume of 10.0M HCl needed to exhaust the remaining capacity of the buffer after the reaction described in part b, we must calculate the moles of H3O+. We start with an initial pH of 1.8 x 10^-5 M HCl, which when converted to moles/L gives us 1.8 x 10^-6 moles. With the addition of 1.0 mL of 0.10 M HCl, we add 1.0 x 10^-4 moles of H3O+. Then the titrant volume is computed, which is 12.50 mL. Remember, since the acid sample and the base titrant are monoprotic and equally concentrated, this titrant addition involves less than a stoichiometric amount of base, hence, it completely reacts with the remaining acid in the solution. For the proper calculation, we convert the 0.500-L volume into milliliters, and we also express the mass percentages as ratios. The final concentration of HCl is computed using the provided volume of HCl solution and the definition of molarity.

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To calculate the mass of 1.32x10^20 uranium atoms, we divide the number of atoms by Avogadro's number to convert atoms to moles. Then, we multiply by the molar mass of uranium to convert moles to grams, which gives us 0.0515 grams.

To calculate the mass of a given number of uranium atoms we first need to know that Avogadro's number (6.02 × 10^23) tells us how many atoms are in one mole of any substance. In this case the molar mass of uranium (U) is 235.04 g/mol.

First, we'll find how many moles 1.32x10^20 atoms represent by dividing by Avogadro's number: (1.32x10^20 atoms) / (6.02x10^23 atoms/mole) which gives us approximately 2.19x10^-4 moles.

Then we multiply this by the molar mass of uranium to get the mass in grams: (2.19x10^-4 mol) * (235.04 g/mol) = 0.0515 grams of uranium.

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The mass of 1.32 x 10²⁰ uranium atoms is approximately 0.0521 grams.

To calculate the mass in grams of 1.32 x 10²⁰ uranium atoms, we need to follow these steps:

1. Determine the molar mass of uranium.

2. Calculate the number of moles of uranium atoms.

3. Convert the moles of uranium atoms to grams.

The molar mass of uranium (U) is approximately 238.03 g/mol.

First, recall Avogadro's number, which is 6.022 x 10²³ atoms/mol. This represents the number of atoms in one mole of any substance.

Number of moles = [tex]\frac{\text{Number of atoms}}{\text{Avogadro's number}}[/tex]

Number of moles = [tex]\frac{1.32 \times 10^{20} \, \text{atoms}}{6.022 \times 10^{23} \, \text{atoms/mol}}[/tex]

Number of moles = [tex]\frac{1.32 \times 10^{20}}{6.022 \times 10^{23}}[/tex]

Let's calculate this:

Number of moles = 2.19 x 10⁻⁴ moles

Now, convert the number of moles to grams using the molar mass of uranium:

Mass (grams) = Number of moles x Molar mass

Mass (grams) = 2.19 x 10⁻⁴ moles x 238.03 g/mol

Mass (grams) = 2.19 x 10⁻⁴ x 238.03

Mass (grams) = 0.0521 grams

Answer:

Equal to

Explanation:

The other person who answered gave a great long explanation, so short answer: Equal to

Final answer:

To confirm the production of carbon dioxide, pass the gas through limewater, which turns cloudy when CO2 is present. For NH3 detection, use red litmus paper, which turns blue, or notice its pungent odor. Ammonia decomposition rates can be used to calculate the production rates of nitrogen and hydrogen.

Explanation:

To verify the production of carbon dioxide in a combustion reaction, you can pass the gas produced through limewater (calcium hydroxide solution). If the limewater turns cloudy, indicating the formation of calcium carbonate, this is a positive test for carbon dioxide. In the case of a decomposition reaction producing NH3, the presence of ammonia can be detected by its characteristic sharp, pungent odor and by using damp red litmus paper, which will turn blue in the presence of NH3.

The rate of decomposition of ammonia (NH3), at a given temperature of 1150 K, can be used to determine the rate of production of nitrogen (N2) and hydrogen (H2). Given the stoichiometry of the balanced equation, which shows that 2 moles of NH3 decompose into 1 mole of N2 and 3 moles of H2, if NH3 decomposes at a rate of 2.10 × 10-6 mol/L/s, then the rate of production of N2 will be half of this rate (1.05 × 10-6 mol/L/s), and the rate of production of H2 will be three times this rate (3.15 × 10-6 mol/L/s).

Answer:

When the forces are weaker, a substance will have higher volatility

Explanation:

Vander Waal's forces are the weakest among the intermolecular forces of attraction. This arises due to the creation of instantaneous dipole moments caused by an instantaneous shift of electrons is a molecule. Stronger the force, stronger will be the interaction between molecules which will in turn be held strongly. When the forces the weaker, the bonds between molecules can be broken easily as a result of which the substance will have a higher volatility.

Answer:

When the forces are weaker, a substance will have higher volatility

Explanation:

b is the correct answer

Answer: The correct answer is True.

Explanation:

Radioactive decay is defined as the process in which an unstable nuclei breaks down into stable nuclei via various methods.

The unstable nucleus is known as parent nuclide and stable nucleus is known as daughter nuclide.

There are many decay processes by which a parent nucleus can undergo decay. They are:

Thus, the correct answer is True.

To subtract 1 from each element in the lowerscores array, you can use a for loop. Within the loop, you can check if the current element is already 0 or negative. If it is, assign 0 to the element. Otherwise, subtract 1 from the element.

To subtract 1 from each element in the lowerscores array, you can use a for loop. Within the loop, you can check if the current element is already 0 or negative. If it is, assign 0 to the element. Otherwise, subtract 1 from the element.

In this example, 'lowerscores' represents the array that contains the scores. The loop iterates through each element of the array and performs the desired subtraction or assignment based on the given condition.

Answer:

0.5421 moles of carbon dioxide are emitted into the atmosphere.

Explanation:

[tex]1C_3H_8 + 5O_2 \rightarrow 3CO2 + 4H2O[/tex]

Moles of octane = [tex]\frac{20.6 g}{114 g/mol}=0.1807 mol[/tex]

According to reaction 1 mol of octane gives 3 moles of carbon dioxide.

Then, 0.1807 moles of octane will give:

[tex]\frac{3}{1}\times 0.1807 mol=0.5421 mol[/tex] of carbon dioxide

0.5421 moles of carbon dioxide are emitted into the atmosphere.