CHEMISTRY HIGH SCHOOL

What element has 3 electrons in its Lewis dot structure and is in the 2p orbital

Answers

Answer 1
Answer: I think the element with 3 electrons in its lewis dot and a 2p orbital will be Boron

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Use the periodic table or graphic in lesson. Choose the correct electron configuration of carbon. 1s22s22p1 1s22s22p4 1s22s22p2 1s22s12p2
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Chlorine and element X have similar chemical properties. An atom of element X could have an electron configuration of(1) 2-2 (2) 2-8-1 (3) 2-8-8 (4) 2-8-18-7

The first major source of oxygen gas was _____.a. volcanic outgassing
b. meteorite impacts
c. cyanobacteria
d. banded iron formations

Answers

The first major source of life on Earth was c. cyanobacteria. These organisms produce food by using energy from the sun; they are photosynthetic organisms. Over millions of years these organisms used CO2 in the air for photosynthesis and released oxygen as a byproduct. Over time oxygen concentrations rose high enough to support life.
The word that best fits in the blank in the sentence, "The first major source of oxygen gas was _____" is cyanobacteria. Thus, the answer is letter C. Cyanobacteria are blue-green algae and they are believed to have caused the "great Oxidation Event".

Which observation illustrates the law of conservation of mass?a. Burning 10 g of propane produces twice as much carbon dioxide as burning 5 g of propane.
b. The C:O mass ratio of one compound is exactly double that of another compound.
c. When 3 g of carbon reacts with 8 g of oxygen, 11 g of carbon dioxide is produced.
d. The C:O mass ratio of a particular compound is the same, regardless of the size or source of the sample.

Answers

I believe that the answer is C. 

Given chemical equations for these reactions s(s) + o2(g)  so2(g) ∆h˚ –296.8 kj•mol–1 h2(g) + ½ o2(g)  h2o(l) ∆h˚ –285.8 kj•mol–1 h2(g) + s(s)  h2s(g) ∆h˚ –20.6 kj•mol–1 what is the value of ∆h for the reaction below? 2 h2s(g) + 3 o2(g)  2 h2o(l) + 2 so2(g) (a) –603.2 kj•mol–1 (b) –562.0 kj•mol–1

Answers

Answer is: enthalpy is -1124 kJ/mol, if we divide reaction with two enthalpy is -562.0 kJ/mol.

Reaction 1: S(s) + O₂(g) → SO₂(g) ΔrH₁ = -296.8 kJ/mol.
Reaction 2: H₂(g) + ½ O₂(g) → H₂O(l) ΔrH₂ = -285.8 kJ/mol.
Reaction 3: H₂(g) + S(s) → H₂S(g) ∆rH₃ = -20.6 kJ/mol.
Reaction 4: 2H₂S(g) + 3O₂(g) → 2H₂O(l) + 2SO₂(g) ΔrH₄ = ?
Using Hess's law reaction number 4 is sum of reaction number 1 multiply with two, reaction number 2 multiply with two and reaction 3 reversed and multiply with two:
ΔrH₄ = 2 · (-296.8 kJ/mol) + 2 · (-285.8 kJ/mol) + 2 · 20.6 kJ/mol.
ΔrH₄ = -1124 kJ/mol.

How many moles of NaCl are present in 23.5 grams of NaCl?

Answers

Answer:

0.342 mol

Explanation:

Molar mass of  

NaCl = 58.4 g/mol

Number of moles in  

20.0 g NaCl

is

20.0

g

58.4

g

/mol

=

0.342 mol

Why do the elements at the bottom of the periodic table have lower ionization energies than their group/family partners at the top of the periodic table?

Answers

Ionization energy is the energy required to remove the losely bounded electron from an isolated gaseous atom of an element, so if an electron is more attracted towards nucleus it will require higher energy. On increasing size of an atom the electrons fall distant from the nucleus and will observe less effective nuclear energy hence less amount of energy will be required to remove them.

On moving down the group, the size of elements increases hence effective nuclear charge will decrease thus ionization energy will decrease.

Elements at the bottom of the periodic table have lower ionization energies compared to their group or family partners at the top of the periodic table because, they have more energy levels.  

Ionization energy decreases down the group as less energy is required to remove outer most electrons as energy levels increases.

Further Explanation

Ionization energy

  • 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.

First ionization energy  

  • 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.

Trend in ionization energy  

1. Down the group (top to bottom)

  • 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.

2. Across the period  (left to right)

  • 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

Learn more about

Level: High school  

Subject: Chemistry  

Topic: Periodic table and chemical families  

Sub-topic: Ionization energy

Mg(s) + 2HCI(aq) -> MgCl2(aq) + H2(g) a. How many grams of HCI are consumed by the reaction of 2.50 moles of magnesium? Given: Requested:

Answers

Answer:2.50 moles of magnesium will consume approximately 182.30 grams of hydrochloric acid in the given reaction.

Explanation:To find out how many grams of hydrochloric acid (HCl) are consumed when 2.50 moles of magnesium (Mg) react with it, you can use stoichiometry and the balanced chemical equation:

Mg(s) + 2HCl(aq) -> MgCl2(aq) + H2(g)

From the balanced equation, you can see that 1 mole of magnesium (Mg) reacts with 2 moles of hydrochloric acid (HCl).

Now, let's use this information to calculate the moles of HCl required to react with 2.50 moles of Mg:

Moles of HCl = (2.50 moles Mg) * (2 moles HCl / 1 mole Mg)

Moles of HCl = 2.50 moles * 2

Moles of HCl = 5.00 moles

Now that we know we need 5.00 moles of HCl, we can calculate the grams of HCl needed using the molar mass of HCl:

The molar mass of HCl is the sum of the atomic masses of hydrogen (H) and chlorine (Cl):

Molar mass of HCl = 1.01 g/mol (for hydrogen) + 35.45 g/mol (for chlorine)

Molar mass of HCl = 36.46 g/mol

Now, calculate the grams of HCl:

Grams of HCl = (5.00 moles) * (36.46 g/mol)

Grams of HCl = 182.30 grams

So, 2.50 moles of magnesium will consume approximately 182.30 grams of hydrochloric acid in the given reaction.
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