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CHE 110 > Exam 2 > Flashcards

Exam 2 Flashcards

1
Q

One half the distance between two nuclei in two adjacent metal atoms
- move across PT, radius decreases
- move down PT, radius increases

A

Atomic radius

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2
Q

The effect in which electrons can reduce the electrostatic attraction between the protons and the nucleus and other protons

A

Shielding

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3
Q

Electrons are shielded very effectively by electrons in sub shells closer to the nucleus
- electrons in the same shell are sheiled only a little
- electrons far way do not shield electrons closer to nucleus

A

Degrees of shielding

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4
Q

Nuclear charge felt by an electron
Electron- sigma

A

Effective nuclear charge

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5
Q

The radius of an anion/cation
-cations are much smaller than their corresponding atoms
- anions are much larger than their corresponding atom

A

Ionic radi

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6
Q

The minimum energy required to remove an electron from a gas atom in a ground state
- positive
- a measure of how tightly the electrons are held in an atom
X- x+ + e-

A

Ionization energy

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7
Q

The energy change that account when an electron is accepted or added by an atom in the gas state to form anion
X- + e- — X-
Halogens want to gain one electron
Large EA means atom wants electrons
Pos or neg
Increases across PT to accept electrons

A

Electron affinity

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8
Q

The easier it is for the electron to be removed the more metallic it is
Increases down period, decreases across

A

Metallic character

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9
Q

Elements with low IE (metals)
Elements with high EA (non metals)
Transfer of electrons and spends time around one nucleus

A

Ionic bonds

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10
Q

Elements with high IE and EA (non metals(
Sharing of electrons and spends time around both nuclei

A

Covalent bond

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11
Q

Elements with high IE and EA (metals)
Delcoalization of electrons and spend time around network of nuclei

A

Metallic bond

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12
Q

Covalent bonds between atoms are strong
Weak attraction between molecules, broken during states, low boiling point, do not conduct electricity

A

Molecular

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13
Q

Contain ions which are strong, electrostatic attraction between ions, these have to be broken up for a state change, high melting and boiling point, does conduct electricity

A

Ionic

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14
Q

What determines which of the types of bonds occur between atoms, the ability of an atom to attract toward itself the two electrons in a chemical bond
Increases up PT as you go across

A

Electronegativity

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15
Q

EN of the atoms are the same, so the shared electrons spend equal time around each nucleus
For example Cl2

A

Non polar covalent

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16
Q

EN of the atoms are not the same, shared electrons spend more time around a certain atom than the other
For example HCL

A

Polar covalent

17
Q

0.0-0.4
Electrons shared equally

A

Non polar

18
Q

0.4-2.0
Electrons shared unequal

A

Polar covalent

19
Q

2.0-3.3
Electrons transferred

A

Ionic

20
Q

Greater polar bond=
Stronger attraction EN=
Less attraction En=

A

Greater difference in EN
Negative
Positive

21
Q

Which group is stable with 6 or 8 electrons

A

Group 13

22
Q

Which period needs a octet

A

2 (C, N, O, F, Ne

23
Q

Who can have more than 8

A

Si, P, S, Cl, Ar, Ge, As, Se, Br, Kr, Sn, Sb, Te, I, Xe

24
Q

Both structures are representations of the true structure of the atom

A

Resonance

25
Q

Structure to show valences

A

Lewis dots

26
Q

Merging the two inaccurate structures into one

A

Resonance hybrid

27
Q

Not a real charge, the difference between the valence electrons in an isolated atom and the number of electrons assigned to the atom in a Lewis structure

Valence e - [ dots + lines]

A

Formal charge

28
Q

The enthalpy change required to break one or multiple bonds in one mole of gaseous molecules

A

Covalent bond energy

29
Q

Order of bond energies

A

Triple is highest
Double
Single

30
Q

Measure of energy contained in the crystal lattice of a compound, equals to the energy that would be released if the component ions were brought together
Distance between charges
Gets smaller as more negative
Energy… more energy means more negative
Increases up and across periodic table

A

Lattice energy

31
Q

Used to determine lattice energy
Application of Hess law
The value of lattice is a large negative number
The formation of ionic compounds is exothermic due to large exothermic value overcoming the positive values of delta H

A

Born haber cycle

CHE 110 (2 decks)

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