Ch. 1: some important things to remember Flashcards

1
Q

organic compounds

A

compounds that contain carbon

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2
Q

atomic number

A

number of protons in the nucleus

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3
Q

mass number

A

protons + neutrons

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4
Q

isotopes

A

same atomic number, but different mass numbers

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5
Q

atomic weight

A

average mass of the atoms in the element

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6
Q

molecular weight

A

sum of the atomic weights off all the atoms in the molecule

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7
Q

what does an atomic orbital tell us?

A

the volume of space around the nucleus where an electron is most likely to be found

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8
Q

minimum energy corresponds to….

A

maximum stability

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9
Q

an atom is most stable if…

A

its outer shell is either filled or contains 8 electrons

if it has no electrons of higher energy

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10
Q

EN is a measure of

A

the ability of an atom to pull its bonding electrons toward itself

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11
Q

electronic configuration describes…

A

the atomic orbitals occupied by the atom’s electrons

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12
Q

a proton is a …..
a hydride ion is…

A

positively charged hydrogen ion

negatively charged hydrogen ion

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13
Q

ionic bond

A

attraction between ions with opposite charges

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14
Q

covalent bond

A

two atoms share a pair of electrons

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15
Q

polar covalent bond

A

covalent bond between atoms with different EN

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16
Q

dipole

A

positive end and a negative end

17
Q

formal charge formula

A

FC = # valence electrons - # of electrons the atom has to itself (lone pair electrons and one half of the bonding electrons)

18
Q

lewis structures show…

A
  • which atoms are bonded
    -lone pairs
    -formal charges
19
Q

when the atom is neutral, how many bonds do C, N, O and H form?

A

C-4
N-3
O-2
H-1

20
Q

carbocation has a

A

positively charged carbon

21
Q

carboanion has a

A

negatively charged carbon

22
Q

sigma bonds

A

single bonds in organic compounds

23
Q

pi bonds

A

side to side overlap of parallel p orbitals

24
Q

bond strength is measured by

A

bond dissociation energy

25
Q

a ___ bond is stronger than a __ bond

A

sigma, pi

26
Q

how does carbon form four bonds?

A

it promotes an electron from an s orbital to an empty p orbital

27
Q

__, __, __ ad halogens form bonds using …

A

C, N, O; hybrid orbitals

28
Q

no pi bonds =

A

sp3 hybridized

29
Q

one pi bond =

A

sp2 hybridized

30
Q

two pi bonds =

A

sp hybridized

31
Q

a double bond consists of

A

one sigma bond and one pi bond

32
Q

a triple bond consists of

A

one sigma bond and two pi bonds

33
Q

the greater the electron density in the region of orbital overlap…

A

the stronger and shorter the bond

34
Q

shorter bond =

A

stronger bond

35
Q
A