Exam 2 Flashcards
Oxoanions
Based on the name of the element that appears before oxygen in its formula with that elements ending changed into ite or ate
Ate has larger number of oxygen atoms than ite
If an element forms more than two oxoanions,the atom with the greatest number of atoms has prefix per and ends in ate
If it’s lower it has the prefix hypo and ends in ite
Bigger-
Per /ate
Lower-
Hypo/ite
polyatomic ions
consist of more than one atom joined by covalent bonds
Acetate
CH3COO−
Carbonate
CO3 2-
Ionization energy
Energy needed to move one mile of electrons from one mile of gas phase atoms or ions
IE
Ionization energy
Neutral atom ionization energy
IE1
First ionization energy values
IE2
Caution with single chargsecind ionization energy values
Electron affinity
The energy change that occurs when one mile of electrons combine with one mile of atoms or ions in the gas phase
EA values for neutral atom are designated for EA1
EA values for an anion with a single charge are designated for EA2
Why does the first ionization energy generally increase across a period for the main group elements
The charge of the nucleus increases across a row and so there is an increase in the attraction between the nucleus and the surrounding areas
Why are the first ionization energies of some of the group 13 elements smaller than the first ionization energies of the nearby alkali earth metals in the same period
It is easier to remove an electron in a p orbital than an s orbital because it experiences less effective nuclear charge
Why are the first ionization energies of some of the group 16 elements smaller than the first ionization energies of the nearby group 15 elements in the same period
There is an enhanced stability in a half filled set of p orbitals
Which are bigger, anions or cations or neutral atoms
Anions tends to be larger than a neutral atom because of the extra electrons
Actions tend to be smaller than the neutral atom because of missing electrons
Z eff (electron affinity)
Typically decreases down a column and increases across a row
What is ionization energy
The energy it takes to remove an electron from the gaseous element
How do you determine which element has the highest ionization energy?
It has the lowest atomic number (smallest size)
How to determine if compound is made of ions
Consist of actions formed by metallic elements and anions formed from nonmetal
Why is there a trend of decreasing atomic size across a period
There is an increase in effective nuclear charge
Electrostatic potential energy
Energy a charged particle has because of its position relative to another charged particle
Directly proportional to the product of the charges of the particle and inversely proportional to the distance between them
Also called Coulombic attraction
E el
Electrostatic potential
Attraction between a positive ion and a negative ion produced ______ E el
Negative
The greater the charges, the shorter the distance between them, and the more negative the E el
Latrice energy and meeting point
The shorter the distance between ions, the greater the lattice energy, and the higher the melting point
Compounds with polyatomic ions are
Classified as ionic
Electron deficient molecules
Be, B, Al
Free radicals
An atom, ion or molecule with an unpaired electron
Length of covalent bond
Equivalent to atoms size
Energy of covalent bond
Longer the covalent bond, smaller the energy
Polarity of covalent bond
Deals with electro negativity. The greater the distance between the numbers, the more polar it is
Steric number
Sum of number of atoms bonded to that atom and the number of lone pairs in it
Bind length is inversely proportional to the ____
Number of bonding interaction.
C-C triple bonds would be shortest and C-C single bonds would be longest
Are the O-N-O bond angles greater in the nitrite ion (NO2) or Nitrate ion (NO3)
Nitrate has the greater bond angle because nitrates line pairs take up more space than bonds
Electro positivity
Realist I’ve measure of an atoms ability to donate electrons in a bind to another atom
Why do the strength of London force generally increase with increasing molecular size
Dispersion forces arise from dipoles caused by the electron distribution being distorted. Larger molecules have more electrons and therefore more distortions and a bigger force
How is it that the dipole moment of HCL is larger than dipole moment of HBr yet HBr boils at a higher temperature?
Both dipole dipole interactions and dispersion forces need to be considered
Do polar bonds cancel on bent structure
No
Two liquids- one polar and one non polar have the same molar mass. Which one had the higher boiling point?
The polar molecules since they have a dipole dipole interaction
If a molecule contains only carbon and hydrogen it is…
Non-polar
What are the diatomic atoms/molecules?
N2, O2, Cl2, F2, H2
What is the electronegativity of non-polar molecules?
Less than .5
If an atom has hydrogen binding, is it polar or non polar?
Polar
What elements does hydrogen bond to in hydrogen bonding
N
O
F
What suffixes are used to show there is oxygen
Ite (less oxygen)
Ate (more oxygen)
Oxyanion
an anion containing one or more oxygen atoms bonded to another element (as in the sulfate and carbonate ions).
Permanent dipole
Separation of electrical charge in a molecule due to unequal distributions of bonding and or lone pairs of e-
Dipole moment (μ)
A measure of the degree to which a molecule aligns itself in an applied electrical feels, a quantitative expression of the POLARITY of a molecule
The more electronegative an element is, the stronger it’s dipole moment
Where does the dipole moment arrow point?
Toward an atom with excess electrical charge
How do you determine if a molecule has an overall dipole
It is necessary to add the individual bond dipoles together to see if they cancel out
