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Thermochemical

NCEA L3 Chem 91390-Demonstrate understanding of thermochemical principles

QuestionAnswer
How many bonding and non-bonding pairs does a trigonal bipyramid molecule have? five bonding and zero non-bonding
How many bonding and non-bonding pairs does a see saw molecule have? four bonding and one non-bonding
How many bonding and non-bonding pairs does a linear molecule have? two bonding and three non-bonding
How many bonding and non-bonding pairs does a T-shaped molecule have? three bonding and two non-bonding
How many bonding and non-bonding pairs does an octahedral molecule have? six bonding and zero non-bonding
How many bonding and non-bonding pairs does a square pyramidal molecule have? five bonding and one non-bonding
How many bonding and non-bonding pairs does a square planar molecule have? four bonding and two non-bonding
what is the buzz light year reference ? si and beyond
What are standard conditions? 1 mole 25c
Fusion meaning? when a solid is changed at its melting point to form a liquid
sublimation meaning? When a solid is converted into a gas
vaporization meaning? When a liquid is converted at its boiling point into a gas
Triangle c H meaning? The enthalpy change when 1 mole of a substance is totally combusted in oxygen under standard conditions.
Triangle f H meaning? The enthalpy change when 1 mole of a substance is formed from its elements in their natural state
What is entropy? A measure of disorder (or randomness) of a system
When does entropy increase? solid to liquid liquid to gas solid dissolved There is also an increase in entropy when a greater number of gas particles form as products than were present as reactants
What causes instantaneous dipoles? They are the result of random rapid motion of the orbiting electrons resulting in at any given time electrons being more concentrated at one end of the molecule forming a partial negative charge for an instant while the other end becomes slightly positive
Why are their differences in the enthalpy values determined through experiment and the theoretical values? Because some of the energy may have been lost to the surroundings and experimental error may account for the rest of the difference in the values.
What is the order of orbital filling for SPDF notation 1s,2s,2p,3s,3p,4s,3d,4p
What are the too anomalies for SPDF notation Cu and Cr
What is the trend for atomic radius across a period? Across a period, atomic radius decreases as the nuclear charge increases and electrons are added to the same energy level and shielding stays the same
What is the trend for atomic radius down a group? Down a group, atomic radius increases because valence electrons are occupying orbitals at higher energy levels so they are further away from the nucleus, so increased shielding
What is the first ionization energy? It is the energy required to remove the least tightly held electron from each atom in one mole of gaseous atoms
Trend for ionization energy on the periodic table? across a period ionization energy increases, and as you go down a group ionization energy decreases.
Electronegativity meaning? Attraction of a bonded atom for a bonding pair of electrons (Increases as you go across period and decreases as you go down group)
While will the cation of an atom have a smaller atomic radius than the atom? Because one or more electrons has been removed from the valence shell so there will be less repulsion between the valence electrons or even has fewer shells so less shielding between valence electrons and protons in the nucelus
What needs to happen for a reaction to be spontaneous? The total entropy change for the system and the surroundings must be positive
Created by: estherbruce
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