Lecture Flashcards

(41 cards)

1
Q

Atomic weight of carbon

A

12.0107

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2
Q

Focus of inorganic chemistry

A

It is the general study of chemicals / elements.

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3
Q

Focus of organic chemistry

A

It is specific to the study of CARBON and to all substances containing it.

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4
Q

Source of molecules in inorg

A

Minerals

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5
Q

Source of molecules in organic chemistry

A

Biological species (animals, plants)

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6
Q

Atomic number gives the ?

A

of protons / electrons

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7
Q

Mass number gives the ?

A

total # of protons and neutrons in the nucleus.

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8
Q

Where can you find the negatively charged electron

A

Within the orbitals

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9
Q

Atomic orbitals is also known as?

A

Wave function

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10
Q

What is atomic orbitals

A

It is the solution to a wave equation — the mathematical expression used to describe the distribution of electrons in an atom.

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11
Q

shape of s orbital

A

Spherical

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12
Q

Shape of p orb

A

Dumbbell shape

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13
Q

Hund’s principle -

A

states that every orbital in a subshell is singly occupied before other orbitals are completely filled and that electrons in a singly occupied orbital will have the same spin

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14
Q

Aufbau’s principle

A
  • states that electrons will fill the lowest available energy level before filling the higher levels
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15
Q

Octet rule

A

states that the valence shell (outermost shell) must be filled completely and must achieve a noble gas configuration (8 valence electron).

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16
Q

Atoms will achieve noble gas configuration by either

A

Forming ionic bond or covalent bond.

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17
Q

Electrons are transferred

18
Q

Electrons are shared

A

Covalent bond

19
Q

Bond between atoms of different
eletronegativity (cations and anions)

20
Q

Bond (occurrence) covalent

A

Between similar atoms and atoms of
nearly equal electronegativity.

21
Q

shows the kernel or nucleus represented by the symbol of the atom surrounded by its valence electrons represented by dots.

A

Lewis dot structure

22
Q

also known as line-bond structures; shows 2- electron covalent bonds as a line and the lone-pair electrons (non- bonding electrons) as dots.

A

Kekúle structure

23
Q

Define electronegativity

A

a measure of the relative attraction an atoms has for the shared electron in a bond.

24
Q

The most electronegative

25
Electronegativity of CNOF
C- 2.5 N- 3.0 O- 3.5 F- 4.0
26
a measure of the degree of inequality in the sharing of electrons between two atoms in a chemical bond.
Bond polarity
27
Non- polar covalent bond
a covalent bond in which there is a equal sharing of electrons between two atoms.
28
is a covalent bond in which there is an unequal sharing of electrons between two atoms.n
Polar covalent bond
29
Electronegativity difference of non polar
0-0.4
30
Electronegativity difference of polar
0.4-1.5
31
the no. of valence electrons in the neutral atom minus the number of covalent bonds to the atom and the number of unshared electrons on the atom.
Formal charge
32
Formula for normal charge
Formal Charge = no . of valence e ! in neutral atom minus (no . of dots + no . of bonds)
33
ground state electron configuration of carbon:
1s2 2s2 2p2
34
Shape of sp3
Tetrahedral 109.5*
35
Shape of sp2
Trigonal planar 120*
36
Shape of sp
Linear 180
37
Overlapping type for sigma bond
Head-on-overlap
38
Overlapping type for pi bond
Sideway overlap
39
forms when 2s orbital hybridize with 3 2p orbitals forming four (4) sp3 hybrid orbitals.
Sp3
40
forms when 2s orbital hybridize with 2 2p orbitals forming three (3) sp2 hybrid orbitals and one (1) unhybridized p-orbital.
Sp2 carbon
41
forms when 2s orbital hybridize with 1 2p orbital forming two (2) sp hybrid orbitals and two (2) unhybridized p-orbitals.
Sp carbon