Why are elements arranged by increasing proton number?
1)So elements in the same group have the same number of outer electrons.2)Only outer shell electrons participate in chemical bonding.3)So elements with similar properties are in the same group.
9 of 22
What happens to the atomic radius across a period?
Atomic radius decreases.
10 of 22
All metals except one are solid at room temperature, what is the exception?
Mercury is liquid at room temperature.
11 of 22
Why do most metals have high melting points?
1)Metals exist as a giant metallic lattice.2)A lot of energy is needed to break the strong metallic bonds in the lattice.
12 of 22
Why are metals good electrical conductors?
1)Metals exist as a giant metallic lattice with delocalised electrons that are free to move and carry charge.
13 of 22
What is monatomic?
Exists as a single atom.
14 of 22
What is diatomic?
Two atoms joined together with a covalent bond.
15 of 22
What are the molecular structures for sulfur and phosphorus?
Sulfur= S8. Phosphorus= P4.
16 of 22
Why do most non-metals have low melting points?
1)Most non-metals have a simple molecular structure.2)Little energy is needed to break weak intermolecular bonds.
17 of 22
Why do most non-metals not conduct electricity?
There are no delocalised electrons to carry charge.
18 of 22
What is the structure of carbon and silicon like?
Giant covalent lattices.
19 of 22
What are the four state symbols and what do they stand for?
Why are most diatomic elements exist as gases at room temperature?
1)All diatomic elements have a simple molecular structure.2)They have low boiling points as little heat energy is needed to break weak intermolecular bonds.
21 of 22
Why do Boron, Carbon and Silicon have high melting points?
1)All exist as giant covalent lattices.2)Large amount of energy is needed to break strong covalent bonds.
22 of 22
Other cards in this set
Card 2
Front
What is a compound?
Back
A substance containing more than one type of atom chemically bonded to each other.
Comments
No comments have yet been made