. For each of the following samples of ionic substances, calculate the number of moles and mass the positive ions present in each sample.

Q: ng sels orbital shown below? A) n = 3, { = 2, ml = -2 %3D B) n = 2, { = 1, ml = -1 C) n = 3, { = 1,…

A: n= principal quantum number denotes size of shell l= azimuthal quantum number denotes no of subshell…

Q: Please provide all the work in detail because I will be using this to study

A: Number of moles of Mg and O can be calculated by the equation given below:

Q: A sample of copper (II) nitrate hydrate has a mass of 1.278 g. The sample is heated until all water…

A: Given , mass of copper (II) nitrate hydrate= 1.278 g        mass of anhydrous copper (II) nitrate  =…

Q: O hydrogen peroxide O tetraphosphorus decoxide O disilicon hexachloride O ammonia

A:

Q: Sort the molecular compounds in the table into groups with the same empirical chemical formula. .…

A: Here we are required to group the compound which have same empirical formula.

Q: calculate the percent of water in the copper (II) sulfate n hydrate by mass. Pentahydrate mass=…

A:

Q: Determine the mass percentage of carbon, C, hydrogen, H, and oxygen, O, in C,H,206. Refer to the…

A: Given molecular formula = C6H12O6 Atomic mass of Carbon (C) = 12.01 g Atomic mass of Hydrogen (H) =…

Q: Predict the charge of the ion formed by each of the following elements. A) Mg, Express your answer…

A: The atoms of elements attain stable noble gas configuration by losing or by gaining of electrons and…

Q: A sample of trifluoroacetic acid, C,HF,O2, contains 72.1 g of fluorine. Calculate the mass of the…

A: 1- First calculate the moles of fluorine atoms :  We know that,  moles of F = ( mass / molar atomic…

Q: Explain what the purpose of a subscription is in a chemical formula

A: The subscript is a number written outside the parentheses (brackets)  in a chemical formula.

Q: ruthenium chloride contains 48.72% ruthenium and 51.27% chlorine by mass. what is the empirical…

A: mass % of ruthenium (Ru) = 48.72 % = 48.72 gmass % of chlorine (Cl) = 51.27 % = 51.27 gEmpirical…

Q: If it is known that a 45.2 mg sample of phosphorus reacts with excess selenium (Se) to form 131.6 mg…

A:

Q: A compound is found to contain 45.71 % oxygen and 54.29 % fluorine by mass. What is the empirical…

A: Let us calculate step by step emphirical formula of given compound.

Q: Tartaric Acid (C4H6O6) is naturally found in fruits like grapes and bananas. It is used in the food…

A: Please find your solution below :

Q: If a compound is composed of 66.71% sulfur and 33.29% oxygen (by mass), the empirical formula of…

A: In empirical formula atoms of compounds are in the ratio of  simplest whole numbers .

Q: 12. Complete combustion of 1.550 grams of a compound produces 1.250 grams of carbon dioxide and…

A: Given data :

Q: The relative numbers of reactants and products are represented by numbers placed to the left of the…

A:

Q: A chemist decomposes samples of several compounds; the masses of their constituent elements are…

A: The mass of constituents are , Na= 10.838 g, S = 7.557 g, O = 15.107 g, Molar masses are, Na=…

Q: Consider a 10.1 g sample of the compound cesium phosphate. Given that you have 0.0205 moles of…

A: Mole concept: The number of molecules or atoms present in the one mole of the substance is equal to…

Q: An unknown compound contains 53.34% rhodium, 9.338% carbon, and the rest is oxygen. a) If you assume…

A: Given a compound with the composition: Rh = 53.34 % C = 9.338 % O = 100 - (53.34 + 9.338) % = 37.322…

Q: osmium by mass. a) If you assume 100.0 g of the compound, what is the mass in grams of osmium that…

A: Since you have posted a question with multiple sub- parts, we will solve first three sub- parts for…

Q: 1.651 g of Silver is combined with 0.1224 g of oxygen. Find the empirical formula.

A: moles of silver combining = mass / atomic mass atomic mass of Ag = 108 g/mol Hence moles of Silver =…

Q: Elemental analysis of putrescine indicates that it consists of 54.0% C, 13.73% H, 31.77% N.…

A: 54.0% C, 13.73% H, 31.77% N.

Q: Consider 1.00 g of Copper (Cu) metal. How many Cu moles are present in this sample? How many Cu…

A: Since moles of element = mass of element / Atomic mass of element  Atomic mass of Cu = 63.5 g/mol…

Q: Given the following imaginary elements and average atomic masses, calculate the molar mass of the…

A: Given compound is A2DR4given atomic mass of A        19.32D         96.18R         20.20X…

Q: Consider a 10.1 g sample of the compound cesium phosphate. a) What is the chemical formula for…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three sub-parts…

Q: salt.

A: Mass of Cupper= 88.81 Mass of Oxygen =100-88.81=11.19 Mole of Cupper =88.81÷63.5= 1.39 Mole of…

Q: How many MOLECULES of dioxygen difluoride are present in 9.22 grams of this compound ?

A: We know, 1 mole of a compound contains 1 Avogadro number of molecules, where 1 avogadro number =…

Q: Calculate the number of moles in a sample of chromium containing 5.00 * 1020 atoms and the mass of…

A:

Q: Complete the following table. Mass of Moles of Sample Molecules in Sample Total Atoms in Sample…

A: Answer shown in attachment provide in explanation box Explanation:

Q: A student, Ken, is given a mixture containing two carbonate compoundscarbonate compounds. The…

A: The given data is as follows- the given mixture is MgCO3 and (NH4)₂CO3 mixture is 69.79% CO3 is by…

Q: Complete the table below for calculating the molar mass of the compound sulfur hexafluoride .…

A: Different type of atoms have different atomic masses and sum of atomic masses present in any…

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates). 

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.