10. The more compact a metal is, the less brittle it becomes. -True? I'm confused about this one because of what the textbook says: "the more compact the atoms become, the harder the metal becomes. While the compactness makes the metal hard, a fracture on any boundary causes the metal to harden even more. This hardening also makes some metal more brittle."

5. How much of a compound would need to be mixed with 114 g of an element if the ratio of the element to the compound is 2 parts element to 1 part compound?

12. What is the major difference between ionic bonding and metallic bonding?
a. In metallic bonding the valence electrons are de-localized
b. In metallic bonding the electrons are held close to the cations
c. In ionic bonding the valence electrons are de-localized
d. In ionic bonding the electrons are held close to the cations
D?

18. When 2 hydrogen gas molecules are combined with 1 oxygen gas molecule, how many water molecules are created?
No idea..

Thanks!

10. The statement in your textbook seems to be contradicting itself a bit, but I can help clarify it for you. When a metal is more compact, meaning its atoms are tightly packed together, it usually becomes harder. This is because the forces between the atoms become stronger, making it more difficult to deform the metal. However, if a fracture occurs in the metal, it can cause the metal to harden even further, making it more brittle. So, while increased compactness generally makes a metal harder, it can also make it more prone to brittleness under certain conditions.

To understand the answer to questions like these, it's important to have a good understanding of the concepts being discussed and to critically analyze the information provided.

5. To determine how much of a compound would need to be mixed with 114 g of an element, you need to use the given ratio of 2 parts element to 1 part compound. This ratio tells you that for every 2 units of the element, you need 1 unit of the compound.

Let's call the amount of compound x. Since the ratio is 2 parts element to 1 part compound, the amount of the element is 2x.

Now, you can set up a proportion to solve for x:

2x / (114 g + x) = 2/1

Cross-multiply and solve for x:

2x = 2(114 g + x)

2x = 228 g + 2x

Subtract 2x from both sides:

0 = 228 g

This equation has no solution, which means that there is no amount of the compound that can be mixed with 114 g of the element to satisfy the given ratio. Therefore, the answer is that no amount of the compound can be mixed with 114 g of the element.

12. The correct answer is a. In metallic bonding, the valence electrons are delocalized. In metallic bonding, positive metal ions (cations) are held together by a "sea" of delocalized electrons that are free to move. This gives metals their unique properties, such as high electrical and thermal conductivity. In ionic bonding, on the other hand, electrons are transferred from one atom to another, resulting in the formation of positively charged cations and negatively charged anions. The electrons in ionic bonding are not delocalized, but rather held close to the cations.

For questions like these, it's important to have a good understanding of the different types of chemical bonding and their characteristics.

18. When 2 hydrogen gas molecules (H2) combine with 1 oxygen gas molecule (O2), they form 2 water molecules (H2O). This reaction is commonly known as the combustion of hydrogen to form water. The balanced chemical equation for this reaction is:

2H2 + O2 -> 2H2O

In this equation, the coefficients (numbers in front of the molecules) represent the number of molecules involved in the reaction. So, 2 molecules of H2 combine with 1 molecule of O2 to form 2 molecules of H2O.