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Description
Flashcards by debostars97, updated more than 1 year ago
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Created by debostars97
over 8 years ago
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| Question | Answer |
| Explain why Se has a smaller atomic radius than K? | Atomic radii decreases across a period. The electrostatic attractions between nucleas and valence electrons increases. Valence electrons are pulled closer to the nuclear. So Se has a smaller nuclear than K. |
| Why does Na have a larger atomic radius than Li? | Valence electrons of Na are in energy levels further away from the nucleas than Li Electrostatic attractions between the nucleas of Na and valence electrons decreases. Therefore the atomic radius of Na is larger than Li |
| Which has the smaller Na+ or Na? | Na loses all of its valence electrons to form Na+ which results in more electron attractions. This results in one fewer level of electrons so Na+ is considerably smaller than Na. |
| Definition for ionization energy is? | The minimum energy needed to remove one electron from each atom in a mole of atoms in the gaseous state. |
| Which is the rule for ionization energy down a group? | Decrease. The electrons lost is further away from the nucleas than the element above. More shielding by the increased number of inner shells. Therefore there is a decrease in electrostatic attraction between nucleas and valence electrons. Less energy is needed to remove the electron. |
| Is the process of ionization energy is endothermic? | No. It is exothermic because energy is required to overcome the electrostatic attractions between the nucleas and the valence electrons |
| Which one had the greatest electronegativity Al or Cl and why? | Cl. Because the bonded electrons are in the same energy level as Al but there is increased positive charge on the nucleas so the attraction increases. So does the electronegativity |
| Identify the forces in H202 | Temporary dipole forces Permanent dipole - permanent dipole Hydrogen bonding. |
| Explain why HCI has a higher boiling point than F2. | F2 has weak temporary dipole-temporary forces which is the weakest intermolecular force so the bonds are easier to break. HCI has permanent dipole - permanent dipole due to the difference in electronegativities. This force is stronger than the weak temporary dipole so it has a higher boiling point. |
| Explain the shape of XeF4. | 6 negative regions arranged in a octahedral arrangement to minimize repulsion. It has 2 lone pairs and therefore it is square planar with a bond angle of 90. |
| Determine the shape of SF4 | Has 5 negative regions arranged in a trigonal bipyramid arrangement yo minimize repulsion. Has one lone pair making the overall shape see - saw. |
| Definition of enthalphy of vaporization | The energy needed to convert 1 mole of liquid to gas at its boiling point. |
| Definition of enthalphy of combustion. | The energy when 1 mole of substance is combusted completely in excess oxygen. |
| Definition of enthalphy of formation. | The energy change when 1 mole of substance is formed from its elements |
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