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Natasha2012 [34]
3 years ago
5

An atom of lithium (Li) forms an ionic bond with an atom of chlorine (Cl) to form lithium chloride. How are the valence electron

s of these atoms rearranged to form this bond? A few valence electrons are shared between the atoms. Many valence electrons are shared between the atoms. Electrons are transferred from the chlorine atom to the lithium atom. Electrons are transferred from the lithium atom to the chlorine atom.
Chemistry
2 answers:
muminat3 years ago
6 0

Answer: Electrons are transferred from the lithium atom to the chlorine atom.

Explanation: Metal atoms tend to give away valence electrons when they bond with nonmetal atoms.

nalin [4]3 years ago
5 0

<u>Answer:</u> The correct statement is electrons are transferred from the lithium atom to the chlorine atom.

<u>Explanation:</u>

Ionic bond is defined as the bond which is formed from the complete transfer of electrons from one atom to another atom. The atom which looses electrons is known as electropositive atom and it attains positive charge. The atom which gains electrons is known as electronegative atom and it attains negative charge.

Lithium is the 3rd element of the periodic table. The electronic configuration of this element is 1s^22s^1

This element will loose 1 electron to attain stable electronic configuration to attain +1 oxidation state.

Chlorine is the 17th element of the periodic table. The electronic configuration of this element is 1s^22s^22p^63s^22p^3

This element requires 1 electron to attain stable electronic configuration to attain -1 oxidation state.

Hence, electrons are transferred from the lithium atom to the chlorine atom.

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If an unknown liquid has a density of 0.756 g/mL and a mass of 2.00 g, what is its volume?
OverLord2011 [107]

Answer:

<h3>The answer is 2.65 mL</h3>

Explanation:

The volume of a substance when given the density and mass can be found by using the formula

volume =  \frac{mass}{density} \\

From the question

mass = 2 g

density = 0.756 g/mL

So we have

volume =  \frac{2}{0.756}  \\  = 2.645502...

We have the final answer as

<h3>2.65 mL</h3>

Hope this helps you

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2 years ago
melting, boiling, and bending are considered physical changes, but burning is a chemical change. explain why this is so.
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3 years ago
Write a chemical equation representing the first ionization energy for lithium. use e− as the symbol for an electron.
just olya [345]

The chemical equation representing the first ionization energy for lithium is given by;

Li → Li + e-

<h2>Further Explanation; </h2><h3>Ionization energy</h3>
  • Ionization energy is the energy required to remove outermost electrons from the outermost energy level. Energy is required to remove an electron from an atom.
  • The closer an electron is to the nucleus the more energy is required, since the electron is more tightly bound to the atom thus making it more difficult to remove, hence higher ionization energy.
  • Ionization energy increases across the periods and decreases down the group from top to bottom.  
  • Additionally, the ionization energy increases with subsequent removal of a second or a third electron.
<h3>First ionization energy  </h3>
  • This is the energy required to remove the first electron from the outermost energy level of an atom.
  • Energy needed to remove the second electron to form a divalent cation is called the second ionization energy.
<h3>Trends in ionization energy  </h3><h3>1. Down the group(top to bottom)</h3>
  • Ionization energy decreases down the groups in the periodic table from top to bottom.
  • It is because as you move down the group the number of energy levels increases making the outermost electrons get further from the nucleus reducing the strength of attraction to the nucleus.
  • This means less energy will be required compared to an atoms of elements at the top of the groups.
<h3>2. Across the period  (left to right)</h3>
  • Ionization energy increases across the period from left to right.
  • This can be explained by an increase in nuclear energy as extra protons are added to the nucleus across the period increasing the strength of attraction of electrons to the nucleus.
  • Consequently, more energy is needed to remove electrons from the nucleus.

Keywords: Ionization energy, periodic table, energy levels, electrons

<h3>Learn more about</h3>
  • Ionization energy: brainly.com/question/1971327
  • Trend in ionization energy: brainly.com/question/1971327
  • First ionization energy: brainly.com/question/1971327

Level: High school  

Subject: Chemistry  

Topic: Periodic table and chemical families  

Sub-topic: Ionization energy

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Answer:

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