Question

Question 1 Write the postulates of Dalton’s theory?

Question 2 Who gave law of conservation of mass?

Question 3 Write the postulate of Dalton’s theory that proves the law of constant proportion?

Question 4 What is chemical formula?

Question 5 What is the Latin name of Sodium, Potassium, tin and lead?

Question 6 What is formula unit?

Question 7 Define one atomic mass unit?

Question 8 What are ions? How is it formed?

Question 9 Calculate the formula mass of Na2CO3∙ 10H2O

Question 10 Write the difference between simple ion and polyatomic ion?

Question 11 Derive formula of aluminum chloride

Question 12 What are ionic compounds?

Question 13 Write the difference between molecule of element and molecule of compound?

Question 14 How Na+

is formed from Na?

Question 15 What is the difference between 2O and O2?

Question 16 Convert 46 gm sodium into moles?

Question 17 Which has more number of atoms 10 gm of sodium or 100 gm of magnesium?

Question 18 Calculate the mass of 2 mole of oxygen?

Question 19 What is Avogadro constant?

Question 20 Write two examples of diatomic molecule?​

Answer 1

Answer:

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Explanation:

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Answer 2

Answer:

• Q1.The atomic theory explains the laws of chemical combination (the Law of Constant Composition and the Law of Multiple Proportions).  Dalton was the first person to recognize a workable distinction between the fundamental particle of an element (atom) and that of a compound (molecule).

• Q2.Antoine Lavoisier A portrait of Antoine Lavoisier, the scientist credited with the discovery of the law of conservation of mass. This law states that, despite chemical reactions or physical transformations, mass is conserved — that is, it cannot be created or destroyed — within an isolated system.
• Q3.The law of multiple proportions, the law of conservation of mass, and the law of constant proportions are not violated by Dalton’s atomic theory. The theory provides a basis to differentiate between elements and compounds.
• Q4. A chemical formula is a way of presenting information about the chemical proportions of atoms that constitute a particular chemical compound or molecule, using chemical element symbols, numbers, and sometimes also other symbols, such as parentheses, dashes, brackets, commas and plus (+) and minus (−) signs.
• Q5. Sodium -  Natrium
• Potassium - Kalium
• Silver - Argentum
• Mercury leaad - Hydragyrum
• Tin - Sannum
• Gold - Aurum
• Q6. A formula unit in chemistry is the empirical formula of any ionic or covalent network solid compound used as an independent entity for stoichiometric calculations. It is the lowest whole number ratio of ions represented in an ionic compound. Examples include ionic NaCl and K₂O and covalent networks such as SiO₂ and C (as diamond or graphite).
• Q7. atomic mass unit A unit of mass equal to 1 / 12 the mass of an atom of the most common isotope of carbon (carbon 12), which is assigned a mass of 12. A hydrogen atom has a mass of 1 atomic mass unit since its mass is 1 / 12 the mass of carbon
• Q8. Ions are formed by the addition of electrons to, or the removal of electrons from, neutral atoms or molecules or other ions; by combination of ions with other particles; or by rupture of a covalent bond between two atoms in such a way that both of the electrons of the bond are left in association with one of the formerly bonded atoms.

Q9. To calculate molar mass of a chemical compound enter its formula and click 'Compute'. In chemical formula you may use:  Any chemical element. Capitalize the first letter in chemical symbol and use lower case for the remaining letters: Ca, Fe, Mg, Mn, S, O, H, C, N, Na, K, Cl, Al.  Functional groups: D, Ph, Me, Et, Bu, AcAc, For, Ts, Tos, Bz, TMS, tBu, Bzl, Bn, Dmg  parantesis () or brackets [].  Common compound names.  Examples of molar mass computations: NaCl, Ca(OH)2, K4[Fe(CN)6], CuSO4*5H2O, water, nitric acid, potassium permanganate, ethanol, fructose.

Q10. A Simple ion is any ion on the periodic table.

a Polyatomic ion contains at least two simple ions buy still only forms one compound.

the main polyatomic ions are:

Acetate: (C2H3COO) with a charge of -1

Hydroxide: (OH) with a charge of -1

Bromate: (BrO3) with a charge of -1

Perchlorate: (ClO4) with a charge of -1

Chlorate: (ClO3) with a charge of -1

Chlorite: (ClO2) with a charge of -1

Hypochlorite: (ClO) with a charge of -1

Cyanide: (CN) with a charge of -1

Nitrate: (NO3) with a charge of -1

Nitrite: (NO2) with a charge of -1

Hydrogen Sulfate: (HSO4) with a charge of -1

Hydrogen Sulfite: (HSO3) with a charge of -1

Sulfate: (SO4) with a charge of -2

Sulfite: (SO3) with a charge of -2

Hydrogen Carbonate: (HCO3) with a charge of -1

Carbonate: (CO3) with a charge of -2

Permaganate: (MnO4) with a charge of -1

Peroxide: (O2) with a charge of -2

Dihydrogen Phosphate: (H2PO4) with a charge of -1

Hydrogen Phosphate: (HPO4) with a charge of -2

Phosphate: (PO4) with a charge of -3

Phosphite: (PO3) with a charge of -3

Chromate: (CrO4) with a charge of -2

Dichromate: (Cr2O7) with a charge of -2

Oxalate: (C2O4) with a charge of -2

Arsenate: (AsO4) with a charge of -3

Ammonium (NH4) with a charge of +1

Ammonium is the only Polyatomic Ion with a positive charge.

Remember to make sure it says (for example) ChlorITE not ChlorIDE when using a Polyatomic ion, because Chloride is Cl and Chlorite is ClO2.

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