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chemistry final > unit 3 > Flashcards

unit 3 Flashcards

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1
Q

electromagnetic spectrum? (highest frequency)

A

gamma rays, x-ray, UV, infrared, microwaves, radio waves.

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2
Q

photoelectric effect?

A

irradiation of clean metal surface with light causes electrons to be ejected from the metal. furthermore, the frequency of the light used for the irradiation must be above some threshold value which is different for every metal.

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3
Q

bohr model - hydrogen?

A

the nucleus is the center of the atom. each orbit has a distinct energy associated with it. the further away from the nucleus the greater the energy.

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4
Q

continuous spectrum?

A

continuous distribution of wavelengths spanning the visible region of electromagnetic spectrum.

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5
Q

line spectrum?

A

a series of discrete lines on an otherwise dark background as a result of light emitted by an excited atom.

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6
Q

de broglie equation?

A

this allows for the calculation of the wavelength of anything from an electron to any other particle or object if you know the mass and velocity.

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7
Q

quantum numbers?

A

wave functions (orbitals) depend on three parameters called quantum numbers.

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8
Q

l - angular-momentum quantum number?

A

defines the three dimensional shape of the orbital and tells us the orbital.

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9
Q

s orbital shape?

A

sphere.

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10
Q

p orbital shape?

A

dumbbell (infinity sign).

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11
Q

d orbital shape?

A

2 dumbbell shapes crossed in the middle (X).

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12
Q

f orbital shape?

A

4 dumbbell shapes crossed multiple times.

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13
Q

ml - magnetic quantum number?

A

defines the spatial orientation of the orbital.

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14
Q

ms - spin quantum number?

A

spinning of electrons gives rise to tiny magnetic fields.

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15
Q

the aufbau principle?

A

electrons fill lower energy levels before higher.

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16
Q

pauli exclusion principle?

A

2 electrons in the same valence shell must be spun up and down.

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17
Q

hund’s rule?

A

in p orbitals etc, each shell must be half filled before fully filled.

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18
Q

anomalies?

A

cu, mo, ag, cr.

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19
Q

effective nuclear charge?

A

extent of shielding. the nuclear charge felt by an electron when both the actual nuclear charge and the repulsive effects (shielding) of the other electrons are taken into account. because core electrons are on average closer to the nucleus than valence electrons, core electrons shield valence electrons to a higher degree than valence electrons shield each other.

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20
Q

effective nuclear charge trend?

A

decreases down a group, increases across a period. atomic size increases across a group therefore increasing electron shielding.

21
Q

atomic radius?

A

decreases across a period, increases down a group.

22
Q

ionic radius?

A

radius of an anion or cation. increases down a group, decreases across a period.

23
Q

ionisation energy?

A

the minimum energy required to remove an electron from a gaseous atom in its ground state.

24
Q

ionisation energy trend?

A

increases across a period, decreases down a group. this is because energy levels increase going down a group and the distance is greater.

25
Q

electron affinity?

A

the negative of the energy change that occurs when an electron is accepted by an atom in the gaseous state to form an ion.

26
Q

electron affinity trend?

A

decreases down a group as atomic radius increases and increases across a period as electrons are added to the energy levels.

27
Q

lewis symbols?

A

electrons involved in bonding are the valence electrons. we show these with lewis symbols.

28
Q

ionic bonds?

A

the ionic bond is an electrostatic force that holds ions together in an ionic compound.

29
Q

lattice energy?

A

the energy required to completely separate one mole of a solid ionic compound into gaseous ions.

30
Q

coulomb’s law?

A

the potential energy between two ions is directly proportional to the product of their charges are inversely proportional to the distance squared between them.

31
Q

covalent bond?

A

a bond where two or more electrons are shared between two atoms.

32
Q

covalent compounds?

A

compounds that contain only covalent bonds.

33
Q

lewis structures p2?

A

a representation of covalent bonding where shared electrons are shown either as lines or as pairs of dots between atoms, and lone pairs are shown as pairs of dots on individual atoms.

34
Q

bond dissociation energy?

A

the energy needed to break a chemical bond in a isolated molecule in the gaseous state. the energy released a bond is formed between gaseous atoms.

35
Q

bond enthalpy?

A

the change in enthalpy required to break a particular bond in one mole of gaseous molecules.

36
Q

bond length?

A

distance between the nuclei of two covalently bonded atoms in a molecule.

37
Q

polar bonds?

A

equal electron sharing between two identical atoms. different atoms desire electrons to varying degrees (electron affinity).

38
Q

polar covalent bond?

A

a covalent bond with greater electron density around one atom than another. polar covalent bonds have unsymmetrical electron distribution in which the bonding electrons are attracted more strongly by one atom than another.

39
Q

electronegativity?

A

electronegativity is a function of an atom’s ability to attract an electrons binding pair.

40
Q

electronegativity trend?

A

increases across a period, decreases down a group.

41
Q

difference in electronegativity?

A

0<0.3 - covalent (non polar)
0.3> and <2.0 - polar covalent
>2.0 - ionic

42
Q

formal charges?

A

an atoms formal charge is the difference between the numbers of valence electrons in an isolated atom and the number of electrons assigned to that atom in a lewis structure.

43
Q

resonance?

A

two of more lewis structures can be accurately drawn to represent a molecule.

44
Q

resonance hybrid?

A

combination of resonance structures?

45
Q

bond strength and highest mp?

A

ionic > polar covalent > non polar

46
Q

trends with common cation?

A

smaller the cation, shorter the distance between nuclei therefore larger lattice energy.

47
Q

examples with common cations - put in order of size: KF NaF LiF?

A

larger the charge, smaller the cation, smaller the distance, larger lattice energy. KF < NaF < LiF

48
Q

common anion?

A

size, smaller the anion, shorter the distance, larger the lattice energy. more core electrons as you go down a group which means more shielding and less attraction of valence electrons.

49
Q

polarity arrows?

A

arrow points towards the more electronegative. arrows never point to hydrogen. arrow points to the sudonegative side of the bond.

chemistry final (4 decks)

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