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Veseljchak [2.6K]
3 years ago
5

Why do all atoms of an element have the same atomic number, although they may have

Chemistry
1 answer:
Evgesh-ka [11]3 years ago
5 0

Answer:

Here’s what I get.

Explanation:

  • The atomic number is the number of protons in the nucleus of an atom.
  • The number of protons determines the number of electrons.
  • The number of electrons determines the chemical properties of the element,

Thus, the atomic number determines the identity of the element.

The atomic mass does not affect the chemical properties, so different isotopes of an element behave alike.

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Which of the following statements correctly describes what happens in all chemical reactions?
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Bonds between atoms are broken/ or new bonds are formed

Explanation:

Due to chemical changes.

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The wave mechanical model of the atom is required to explain the
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The wave-mechanical model of the atom is required to explain the spectra of elements with multi electron atoms.

<u>Explanation:</u>

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2. How many chlorine atoms are in 4 moles of chlorine?
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Answer:

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A chemist adds of a M barium acetate solution to a reaction flask. Calculate the mass in grams of barium acetate the chemist has
tekilochka [14]

Complete Question:

A chemist adds 55.0 mL of a 1.1M barium acetate (Ba(C2H3O2)2) solution to a reaction flask. Calculate the mass in grams of barium acetate the chemist has added to the flask. Round your answer to 2 significant digits.

Answer:

15 g

Explanation:

The concentration of the barium acetate is given in mol/L (M), thus, the number of moles (n) of it is the concentrantion multiplied by the volume (55.0 mL = 0.055 L):

n = 1.1 * 0.055

n = 0.0605 mol

The molar mass of the substance can be calculated by the sum of the molar mass of each element, which can be found at the periodic table. Thus:

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C = 12.00 g/mol

H = 1.00 g/mol

O = 16.00 g/mol

Ba(C2H3O2)2 = 137.33 + 4*12 + 6*1 + 4*16 = 255.33 g/mol

The molar mass is the mass divided by the number of moles, thus the mass (m) is the molar mass multiplied by the number of moles.

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