Classify these bonds as ionic, polar covalent, or nonpolar covalent na-f

Since it has a 4 protons and 5 neutrons, it has a mass number of 9. The number of electrons is irrelevant for this question. Atomic number is the number of protons, so it is 4. So it is Beryllium

Answer:

Is your answer right or are you asking a question??

Answer:

It's the metal that gets named first.

Explanation:

Compounds are named based on the ions they produced on dissolution. In a compound that contains monatomic ions, the metallic ion is a named first. Thus 4th option is correct.

A monatomic ion is a single atom possessing a positive charge or negative charge. The ion bearing a positive charge is called cation and the ion bearing negative charge is called anion.

Cations are formed by the losing or donation of electrons. Whereas, anions are formed by withdrawal of electrons. For example Na+ is a cation and Cl- is an anion formed by losing of one electron from sodium metal and accepting an electron Cl gas respectively.

These single atomic  cation and anions together forms ionic compounds called monatomic ions. For example NaCl containing sodium ion and chloride Cl- ion is a monatomic ion and its name is started with the metal sodium namely sodium chloride.

Similarly HBr containing H + ion and Br- ion have the name hydrogen bromide. Therefore, the metal named first for a compound containing monatomic ions.

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To form 14.6 grams of iron(iii) oxide, or rust, about 4.4 grams of oxygen are required, based on the stoichiometry of the rust-forming reaction.

The formation of rust, or iron(iii) oxide, involves the reaction of iron with oxygen. To determine the amount of oxygen needed for this process, we need to understand the stoichiometry of the reaction. Two moles of iron react with one mole of oxygen to produce two moles of iron(iii) oxide. The molar mass of iron (Fe) is approximately 56 g/mol, of oxygen (O) is about 16 g/mol, and Iron(III) Oxide (Fe2O3) is ~160 g/mol.

To calculate the grams of oxygen needed for 14.6 g of rust (Fe2O3), you first convert the given mass of iron(iii) oxide into moles, then use the stoichiometry of the reaction to determine how many moles of oxygen are required.

14.6g Fe2O3 * (1 mol Fe2O3/160 g) = 0.09125 mol Fe2O3

The reaction indicates that for every 1 mole of Fe2O3 produced, 1.5 moles of oxygen(O2) are needed. So:

0.09125 mol Fe2O3 * (1.5 mol O2/1 mol Fe2O3) = 0.137 mol O2

Finally, convert moles of oxygen into grams:

0.137 mol O2 * (32 g/mol) = approximately 4.4 grams

So, for 14.6g of Fe2O3 to form, around 4.4 g of O2 are needed.

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To produce 14.6 g of iron(III) oxide, approximately 4.39 grams of oxygen are needed. The nearest answer is option b. 4.4 g

The calculation involves converting grams to moles, using the stoichiometric ratio from the balanced equation, and then converting back to grams.

To determine how many grams of oxygen are needed for the reaction, we start with the balanced chemical equation for the formation of iron(III) oxide (rust):

We know that 14.6 g of Fe₂O₃ is produced.

The molar mass of Fe₂O₃ is calculated as follows:

Next, we convert 14.6 g of Fe₂O₃ into moles:

According to the balanced equation, 2 moles of Fe₂O₃ are produced from 3 moles of O₂. Thus, the moles of O₂ needed are:

Finally, we convert moles of O₂ to grams of O₂ using the molar mass of O₂ (32.00 g/mol):

Therefore, approximately 4.39 grams of oxygen are needed to produce 14.6 g of iron(III) oxide.

Correct question is: Consider the reaction 2Fe(s) + 30₂ (g) ► Fe₂O₃(g) . If 14.6 g of iron(III) oxide (rust) is produced from a certain amount of iron, how many grams of oxygen are needed for this reaction?

a. 1.85 g

b. 4.4 g

c. 3.74 g

d. 2.68 g

add them all together then divide it by the amount that Is their

The molarity of chloride ions in the final solution is equal to 0.156 M.

Molarity can be defined as the concentration of the solution in terms of moles of solute and volume of solution in liters.

Given the solution of calcium chloride:

[tex]CaCl_2 \longrightarrow Ca^{2+} + 2Cl^{-}[/tex]

Given the molarity of calcium chloride  = 0.1 M

The concentration of chloride ions in the solution = 2×0.1 = 0.2 M

The volume of solution, V = 50 ml = 0.05 L

The number of moles of chloride = 0.2× 0.05 = 0.001 mol

Amount of NaCl added in the solution = 0.400 g

The number of moles of chloride from NaCl = 0.4/58.5 = 0.0068 mol

Total number of moles of chloride ions = 0.001 + 0.0068 = 0.0078 mol

Volume of the whole solution = 50 ml = 0.05 L

The molarity of the chloride ions in the final solution:

M = 0.0078/0.05

Molarity = 0.156 M

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Cr and O are most likely to be part of a polyatomic ion.

Cr belongs to the transition metal series in the periodic table and has vacant d-orbitals. As a result it can exist in more than one oxidation state, the most common being +6, +3 and +2. Oxygen exists in -2 oxidation state. Hence, Cr and O can combine to form different polyatomic ions like: CrO₄²⁻ and Cr₂O₇²⁻ (Cr in +6 state)

K, Li and Mg exist in only one oxidation state +1 (K and Li) and +2(Mg). F and Br exhibit an oxidation state of -1. Therefore, they are not likely to form polyatomic ions.

Ans (a) Cr and O

The formula Ca(ClO3)2 breaks down to 1 calcium atom, 2 chlorine atoms, and 6 oxygen atoms. One molecule of calcium chlorate contains 9 atoms. Thus the correct option is A.

Calcium chlorate is formed by passing chlorine gas through a hot suspension of calcium hydroxide in water, producing calcium hypochlorite, which disproportionate when heated with excess chlorine to give calcium chlorate and calcium chloride.

6 Ca(OH)2 + 6 Cl2 → Ca(ClO3)2 + 5 CaCl2 + 6 H2O

This is also the first step of the Liebig process for the manufacture of potassium chlorate. Liebig's method is used for the estimation of carbon and hydrogen.

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The chemical formula for the compound formed between sodium and oxygen is Na₂O, which is known as sodium oxide. Sodium reacts with oxygen to form this ionic compound.

The compound that is formed when sodium and oxygen combine is known as sodium oxide. Its chemical formula is Na₂O. Sodium (Na) and oxygen (O₂) react together to form this compound. Sodium is a soft, silvery-white metal which reacts vigorously with oxygen to form Na₂O. Oxygen, a gas under standard conditions, reacts with sodium to form an ionic compound with properties entirely different from the constituent elements. Sodium oxide is a white, crystalline solid that is often used in ceramics and glasses.

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HCl = 0.1 M. 

find grams of Acid to neutralize the tablet. 

n = 0.00739 mol of CO3-2. 

D = 1.02 g/ml. 

Find the moles of CO3-2.

CO3-2 + 2HCl <---> H2CO3 + 2Cl-.

therefore,

we need 2 mol of CO3-2 to neutralize 1 mol of HCl.

since we have 0.00739 mol of CO3-2, that will neutralize 2X mol of HCl.

2*0.00739 = 0.01478 mol of HCl will be neutralized.

Now, find the mass of Acid :

M = mol/V,

V = mol/M.

Substitute data of acid :

V = 0.01478 mol / 0.1 M = 0.1478 Liters of stomach acid

or 147.8 ml of stomach acid

now find mass:

D = mass/V.

mass = D*V = 1.02*147.8 = 150.76 grams of Stomach Acid will be neutralized

The spectator ions in this reaction is C) K⁺ and Br⁻

The spectator ions in the given reaction are K⁺ and Br⁻ because they remain unchanged on both sides of the equation.

In the given reaction :

We need to identify the spectator ions.

Thus, the correct answer is:C) K⁺ and Br⁻

To determine the grams of H2 gas produced from the given mass of Al, we use stoichiometry and the molar mass of H2.

To determine the number of grams of H2 gas that can be produced, we need to use the given information about the mass of Al and the balanced chemical equation.

First, we calculate the number of moles of Al by dividing the mass of Al by its molar mass. Then we use the stoichiometric ratio from the balanced equation to find the moles of H2 gas produced. Finally, we convert moles of H2 gas to grams using the molar mass of H2.

By following these steps, we can calculate the grams of H2 gas produced from the given mass of Al.

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By reacting 63.0 grams of Al with excess hydrochloric acid, approximately 7.07 grams of H₂ gas will be produced.

This is based on stoichiometric calculations using a balanced chemical equation.

Given that we have 63.0 grams of Al, we start by converting this mass to moles:

Step 1: Calculate moles of Al

Step 2: Use the mole ratio to find moles of H₂ produced

Step 3: Convert moles of H₂ to grams

Therefore, 6.99 grams of H₂ gas can be produced by reacting 7.07 grams of Al with an excess of dilute hydrochloric acid.

Correct question is: How many grams of H₂ gas can be produced by the reaction of 63.0 grams of Al(s) with an excess of dilute hydrochloric acid in the reaction shown below?

2 Al(s) + 6 HCl(aq) → 2 AlCl₃(aq) + 3 H₂(g)

Answer:

The correct answer is because they work at different pH levels.

Explanation:

The pH varies because the different enzymes secreted in the stomach work at different pH levels. Gastric secretion is the most important stage of digestion since when the food comes into contact with a low pH and the enzymes present, they dissociate it and denature the proteins present.

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An imbalanced chemical equation describes the products and reactants of a chemical reaction.  Therefore, the balanced equation is 2Fe(HCO[tex]_3[/tex])[tex]_3[/tex]+ 3CaO →Fe[tex]_2[/tex]O[tex]_3[/tex]+3Ca(HCO[tex]_3[/tex])[tex]_2[/tex].

A balanced equation is indeed a chemical reaction equation in which the overall charge and the amount of atoms for every element inside the reaction are the same for both the products and the reactants. In other terms, the mass as well as charge on the both sides of both the reaction are balanced.

An imbalanced chemical equation describes the products and reactants of a chemical reaction yet does not include the quantities needed to meet mass conservation.

Fe(HCO[tex]_3[/tex])[tex]_3[/tex]+ CaO →Fe[tex]_2[/tex]O[tex]_3[/tex]+Ca(HCO[tex]_3[/tex])[tex]_2[/tex]

The atom of Fe on reactant side is 1 while on product side it is 2

2Fe(HCO[tex]_3[/tex])[tex]_3[/tex]+ 3CaO →Fe[tex]_2[/tex]O[tex]_3[/tex]+3Ca(HCO[tex]_3[/tex])[tex]_2[/tex]

Therefore, the balanced equation is 2Fe(HCO[tex]_3[/tex])[tex]_3[/tex]+ 3CaO →Fe[tex]_2[/tex]O[tex]_3[/tex]+3Ca(HCO[tex]_3[/tex])[tex]_2[/tex].

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Answer:

You can separate the mixture to collect the iron using a magnetic.

Explanation:

The printing on the box claims that your cereal has the most metallic iron of any breakfast cereal on the planet.

The last sample of the breakfast cereal contains bran flakes, raisins, milk and sugar. We need to analyze the iron content.

There are several chemical and physical experiments about this topic, the simplest is: You can use a magnetic material, the magnetic field of the material will affect the mixture previously prepared. In that way, only the metallic iron will move with the magnetic field movements. So, you can separate the metallic iron from all the other compounds. 

Final answer:

A lamp with an incandescent bulb is less efficient as it converts more electrical energy to heat, whereas a TV uses energy more effectively for display and sound. Employing more efficient lighting such as fluorescent or LED bulbs can significantly reduce energy usage and costs.

Explanation:

Differences in Electrical Energy Use Between Lamps and TVs

When comparing the use of electrical energy between different appliances such as a lamp and a TV, it is important to consider their power consumption and efficiency. A lamp, especially if it uses an incandescent bulb, tends to be less efficient as it loses most of its energy as heat rather than light. On the other hand, a TV is designed to convert electrical energy into both light (the visual part of the display) and sound, typically using the energy more efficiently regarding the provision of its intended service.

To reduce electrical energy consumption and its associated costs, one can switch from incandescent bulbs to fluorescent lights or LED lights, which are more efficient. Fluorescent lights are about four times more efficient than incandescent lights, and LEDs are even more efficient than CFLs. Considering that a significant percentage of energy use in homes and businesses goes to lighting, switching to more efficient lighting options presents a valuable opportunity for energy and cost-saving.

For example, one could replace a 60-W incandescent bulb with a 15-W CFL that provides the same brightness and color. This change not only reduces power consumption but also lowers heat transfer and environmental impact since CFLs have a longer lifespan. LED lights offer improvements over CFLs in both efficiency and lifespan, but their higher cost might be a barrier, although prices have been decreasing over time.

Final answer:

To determine the molecular formula, calculate the moles of carbon and hydrogen from their masses, find the simplest whole-number ratio for the empirical formula (CH3), and then determine how many times the molar mass of the empirical formula fits into the molar mass of the compound to get C2H6.

Explanation:

The question involves determining the molecular formula of a compound from its percent composition by mass and its molar mass. Given that the compound is 80.0% carbon and 20.0% hydrogen by mass, and assuming a 100 g sample, we would have 80.0 g of carbon and 20.0 g of hydrogen. The molar mass of carbon is approximately 12.01 g/mol, and hydrogen is approximately 1.008 g/mol. Therefore, we can calculate the moles of carbon and hydrogen:

The ratio of carbon to hydrogen moles is approximately 1:3. To determine the simplest whole-number ratio, we divide each by the smallest number of moles, which in this case is the moles of carbon, getting exactly 1 C and 3 H. This gives us the empirical formula CH3. To find the molecular formula, we divide the molar mass of the compound by the molar mass of the empirical formula:

Molar mass of CH3 = 12.01 g/mol + (3 × 1.008 g/mol) = 15.034 g/mol

Molecular formula determination:

30.069 g/mol (molar mass of compound) ÷ 15.034 g/mol (molar mass of empirical formula) = 2

Therefore, the molecular formula is C2H6, as we multiply the subscripts in the empirical formula by 2.

4.02 atm

Given:  

SO₂ (5.00 g) and CO₂ (5.00 g) were placed in a 750.0 ml container at 50.0°C.

Question:  

The partial pressure of CO₂ in the container was ... atm.

The Process:

This problem is only required to find the partial pressure of CO₂ in containers, so we ignore SO₂ in the calculation.

Step-1: preparing for the molar mass of carbon dioxide

Mr CO₂ = 12 + 2(16) = 44 g/mol

Step-2: find out the number of mole of CO₂

Mole conversions [tex]\boxed{ \ moles = \frac{mass}{Mr} \ }[/tex]

Therefore, moles of CO₂ = [tex]\boxed{ \ moles = 5.00 \ g \times \frac{1 \ mol}{44 \ g} \ } \rightarrow \boxed{ \ = 0.11364 \ moles \ }[/tex]

Step-3: find out the partial pressure of CO₂ (in atm)

We use an equation of state for an ideal gas:  

[tex]\boxed{\boxed{ \ \frac{pV}{T} = nRT \ }}[/tex]  

Prepare p as the subject you want to find.

[tex]\boxed{ \ p = \frac{nRT}{V} \ }[/tex]

[tex]\boxed{ \ p = \frac{0.11364 \times 0.0821 \times 323}{0.75} \ }[/tex]

Thus the partial pressure of CO₂ in the container was 4.018 atm, rounded up to 3 significant digits, we get 4.02 atm.

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