Term
| the compounds Na20, Al2O3, and SO2 are what in terms of acidity? |
|
Definition
| basic, amphoteric, and acidic |
|
|
Term
| name two properties that are typical of most non-metals in period 3 |
|
Definition
| they form ions by gaining on or more electrons;they are poor conductors of heat and electricity; |
|
|
Term
| describe the trends of melting point from Li to Cs and F to I? |
|
Definition
| decreasing and increasing |
|
|
Term
| state and explain the trend in electronegativity across period 3 from Na to Cl (2) |
|
Definition
electronegativity increases from left to right across period 3;
nuclear charge increases while energy level remains the same, electron affinity increases; |
|
|
Term
| why would Cl2 react more vigorously with a solution of I- than Br2 (2) |
|
Definition
Cl2 has a higher electron affinity than Br2;
Cl2 would pull the electron from I- |
|
|
Term
| explain, in terms of their structure and bonding, why the element sulfur is a non-conductor of electricity and aluminum is a good conductor of electricity (4) |
|
Definition
high ionic character determines good conductivity;
sulfur forms a molecular covalent structure with no ionic character;
aluminum forms a giant ionic structure;
aluminum has delocalized electrons; |
|
|
Term
| Explain, in terms of its structure and bonding, why silicon dioxide SiO2 has a high melting point (2). |
|
Definition
SiO2 forms a giant covalent structure;
its bonds are very strong and hard to break; |
|
|
Term
| suggest why more energy is needed to remove an electron from Na+ than from Mg+ |
|
Definition
| the electron in Na+ is in a closer energy level to the nucleus, so the nucleus as a much greater pull on it |
|
|
Term
write the equation for each reaction between water and
Sodium Oxide
sulfur dioxide |
|
Definition
Na2O+ H20 ==> 2NaOH
SO2 + H20 ==> H2S03 |
|
|
Term
| describe the trends in atomic radii, ionic radii, first ionization energies, electronegativities, and melting points for Li==>Cs |
|
Definition
atomic radii: increase
ionic radii: increase
first ionization energies: decrease
electronegativies: decrease
melting points: decrease |
|
|
Term
| describe the trends in atomic radii, ionic radii, first ionization energies, electronegativities, and melting points for F==>I |
|
Definition
atomic radii: increase
ionic radii: increase
first ionization energies: decrease
electronegativies: decrease
melting points: increase |
|
|
