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Chem > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

Oxoanions

A

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

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2
Q

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

A

Bigger-

Per /ate

Lower-

Hypo/ite

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3
Q

polyatomic ions

A

consist of more than one atom joined by covalent bonds

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4
Q

Acetate

A

CH3COO−

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5
Q

Carbonate

A

CO3 2-

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6
Q

Ionization energy

A

Energy needed to move one mile of electrons from one mile of gas phase atoms or ions

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7
Q

IE

A

Ionization energy

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8
Q

Neutral atom ionization energy

A

IE1

First ionization energy values

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9
Q

IE2

A

Caution with single chargsecind ionization energy values

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10
Q

Electron affinity

A

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

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11
Q

Why does the first ionization energy generally increase across a period for the main group elements

A

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

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12
Q

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

A

It is easier to remove an electron in a p orbital than an s orbital because it experiences less effective nuclear charge

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13
Q

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

A

There is an enhanced stability in a half filled set of p orbitals

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14
Q

Which are bigger, anions or cations or neutral atoms

A

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

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15
Q

Z eff (electron affinity)

A

Typically decreases down a column and increases across a row

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16
Q

What is ionization energy

A

The energy it takes to remove an electron from the gaseous element

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17
Q

How do you determine which element has the highest ionization energy?

A

It has the lowest atomic number (smallest size)

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18
Q

How to determine if compound is made of ions

A

Consist of actions formed by metallic elements and anions formed from nonmetal

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19
Q

Why is there a trend of decreasing atomic size across a period

A

There is an increase in effective nuclear charge

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20
Q

Electrostatic potential energy

A

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

21
Q

E el

A

Electrostatic potential

22
Q

Attraction between a positive ion and a negative ion produced ______ E el

A

Negative

The greater the charges, the shorter the distance between them, and the more negative the E el

23
Q

Latrice energy and meeting point

A

The shorter the distance between ions, the greater the lattice energy, and the higher the melting point

24
Q

Compounds with polyatomic ions are

A

Classified as ionic

25
Q

Electron deficient molecules

A

Be, B, Al

26
Q

Free radicals

A

An atom, ion or molecule with an unpaired electron

27
Q

Length of covalent bond

A

Equivalent to atoms size

28
Q

Energy of covalent bond

A

Longer the covalent bond, smaller the energy

29
Q

Polarity of covalent bond

A

Deals with electro negativity. The greater the distance between the numbers, the more polar it is

30
Q

Steric number

A

Sum of number of atoms bonded to that atom and the number of lone pairs in it

31
Q

Bind length is inversely proportional to the ____

A

Number of bonding interaction.

C-C triple bonds would be shortest and C-C single bonds would be longest

32
Q

Are the O-N-O bond angles greater in the nitrite ion (NO2) or Nitrate ion (NO3)

A

Nitrate has the greater bond angle because nitrates line pairs take up more space than bonds

33
Q

Electro positivity

A

Realist I’ve measure of an atoms ability to donate electrons in a bind to another atom

34
Q

Why do the strength of London force generally increase with increasing molecular size

A

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

35
Q

How is it that the dipole moment of HCL is larger than dipole moment of HBr yet HBr boils at a higher temperature?

A

Both dipole dipole interactions and dispersion forces need to be considered

36
Q

Do polar bonds cancel on bent structure

A

No

37
Q

Two liquids- one polar and one non polar have the same molar mass. Which one had the higher boiling point?

A

The polar molecules since they have a dipole dipole interaction

38
Q

If a molecule contains only carbon and hydrogen it is…

A

Non-polar

39
Q

What are the diatomic atoms/molecules?

A

N2, O2, Cl2, F2, H2

40
Q

What is the electronegativity of non-polar molecules?

A

Less than .5

41
Q

If an atom has hydrogen binding, is it polar or non polar?

A

Polar

42
Q

What elements does hydrogen bond to in hydrogen bonding

A

N

O

F

43
Q

What suffixes are used to show there is oxygen

A

Ite (less oxygen)

Ate (more oxygen)

44
Q

Oxyanion

A

an anion containing one or more oxygen atoms bonded to another element (as in the sulfate and carbonate ions).

45
Q

Permanent dipole

A

Separation of electrical charge in a molecule due to unequal distributions of bonding and or lone pairs of e-

46
Q

Dipole moment (μ)

A

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

47
Q

Where does the dipole moment arrow point?

A

Toward an atom with excess electrical charge

48
Q

How do you determine if a molecule has an overall dipole

A

It is necessary to add the individual bond dipoles together to see if they cancel out

Chem (18 decks)

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