Answer:
1. How many electrons does hydrogen need in order to have a full shell of valence electrons?...two
2. How do valence electrons impact the type of bonds an atom makes?...An atom wants a full outer shell of valence electrons, so it will either transfer or share electrons depending on what the other atom needs.
3.Use your knowledge of valence electrons and how they affect bonds to figure out how carbon (Group 14) and oxygen (Group 16) would be attached to one another. In carbon dioxide (CO2), how is the compound structured? (Use “–” to represent a single bond and “=” to represent a double bond.)...O=C=O
4. Methane’s chemical formula is CH4. Is there a bond between any of the hydrogen atoms? Why or why not?...No, there is not because carbon needs four bonds, so it bonds with each hydrogen atom; hydrogen only forms one bond.
5. In hydrogen peroxide (H2O2), which option best shows how the atoms are ordered?...H-O-O-H
Explanation:
If the water molecule was linear instead of bent the water would no longer produce hydrogen bonds.
<u>Explanation:</u>
- Yes, If the water molecule was linear instead of bent the water would no longer produce hydrogen bonds.
- The water would no longer generate hydrogen bonds.
- It will lose its polar features and nearly all of its features will change such as boiling point, water tension and solubility.
- It would be more like to gas, rather than liquid.
- If the water was in the linear, the water would have all the features and it would produce the hydrogen bonds.
The balanced equation is as below
2 N₂O₃ → 2N₂ + 3O₂
<u><em> Explanation</em></u>
According to the law of mass conservation the number of atoms in reactants side must be equal the to the number of atoms in products side.
Therefore the balanced reaction above is balanced since the number of atoms in reactants side are equal to number of atoms in products side.
For there 4 atoms of N in reactants side and 4 in products side.
Answer:
C: object does not slide off the pan
Explanation:
160 g of SO3 are needed to make 400 g of 49% H2SO4.
<h3>How many grams of SO3 are required to prepare 400 g of 49% H2SO4?</h3>
The equation of the reaction for the formation of H2SO4 from SO3 is given below as follows:
1 mole of SO3 produces 1 mole of H2SO4
Molar mass of SO3 = 80 g/mol
Molar mass of H2SO4 = 98 g/mol
80 g of SO3 are required to produce 98 og 100%H2SO4
mass of SO3 required to produce 400 g of 100 %H2SO4 = 80/98 × 400 = 326.5 g of SO3
Mass of SO3 required to produce 49% of 400 g H2SO4 = 326.5 × 49% = 160 g
Therefore, 160 g of SO3 are needed to make 400 g of 49% H2SO4.
Learn more about mass and moles at: brainly.com/question/15374113
#SPJ1
