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Chemistry > Test (Chapters up till 7) > Flashcards

Test (Chapters up till 7) Flashcards

introduction chapter

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1
Q

Who was george stahl? What theory did he propose? How does it work

A

George Stahl proposed phlogiston theory. Phlogiston flowed out of burning material. Burning stop when air became saturated w/ phlogiston.

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2
Q

what did Joseph priestly discover? What did he name it?

A

Oxygen. Named it dephlogisticated air.

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3
Q

Who was Antoine Lavoisier?

A

Father of modern chemistry. Disproved phlogiston theory. Explained combustion and stated it supports life. Published first modern book: elementary treatise on chemistry.

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4
Q

What law did Joseph Proust create? What is it?

A

Law of constant composition (or definite proportion). a given compound always has exactly the same proportion of elements by mass.

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5
Q

What law did John dalton propose? What was it

A

Law of multiple proportion. If elements combine in different ratios, they are always whole numbers.

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6
Q

Name all 4 parts of daltons atomic theory?

A
  1. each element is made of atoms
  2. atoms of given elements are identical
  3. chemical compounds are formed when elements combine. A combine always has the same relative # of atoms
  4. Chemical Reactions are reorganizations of atoms
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7
Q

What else did John dalton do?

A

Constructed a table of masses. Many were wrong but it was an important step in creating the periodic table

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8
Q

Joseph Gay Lussac and Amadeo Avogadro- What did they do?

A

determined formulas for compounds, gay-lussac measured volume of gases that reacted with each other at constant temp and pressure. Avogadro’s hypothesis interpreted lussacs experiments and proposed that a tthe same temp and pressure, equal volumes of different gasses contain the same number of particles.

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9
Q

What are all of the diatomic molecules?

A

H2, N2, O2, F2, Cl2, Br2, I2

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10
Q

What did Berzelius do?

A

discovered 4 elements, created a symbol system for elements, determined atomic mass of 50 known elements, and performed over 2000 experiments in 10 years.

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11
Q

Who was JJ Thomson?

A

discovered electrons

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12
Q

what is electrons charge to mass ratio?

A

e/m= 1.76*10^8 (C/g) *coulombs per gram

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13
Q

Plum Pudding Model?

A

since atoms are electrically neutral, atoms must be positive. The diagram was a positive cloud with electrons scattered inside of them.

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14
Q

Gold foil experiment?

A

determined positive charge was central

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15
Q

Oil drop experiment

A

Robert Millikan performed it to measure charge of an electron. Used charge to mass ratio.

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16
Q

Mass of an electron?

A

9.10*10^-28 (g)

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17
Q

Who was Henri Becquerel? What did he do? Who was Marie Curie? What did she do?

A

Henri saw a rock leaving an image on a photographic plate in absence of light. Marie curie coined it radioactivity. She later identified other radioactive elements. Won nobel prize for chem.

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18
Q

What is radiation? What are the 3 types?

A

It is spontaneous emission of radiation. Gamma rays are high speed energy (light/photon), Beta particles are high speed electrons, and aplha particles are helium ions (w/ no e-).

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19
Q

What are isotopes?

A

Atoms w/ different numbers of neutrons. Identical chemical properties. In nature, most elements are mixtures of isotopes.

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20
Q

What is counting by weighing?

A

Weigh a small sample, calculate the mass per unit, then weigh a larger sample and find the number of units.

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21
Q

how many g in one amu?

A

1.66*10^-24 (g)

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22
Q

What does a mass spectrometer do?

A

most accurate machine for atomic weighing.

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23
Q

Know how to calculate avg atomic mass

A
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24
Q

Avogadros number?

A

6.022*10^23

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25
Q

Know stoichiometry

A
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26
Q

Know % mass composition

A
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27
Q

Know how to find molecular formula from empirical formula

A
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28
Q

Know how to detrmine an empirical formula from a given mass

A

obtain masses. Calculate mass by % of each element. Assume 100g of compound. Calculate moles of each element. Calculate rations.

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29
Q

What is the Bohr Model?

A

Proposed electrons move in orbits rather than rings

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30
Q

Energy Equation from Bohr’s Model?

A

E= -2,178*10^-18 [Z^2/N^2] where e is energy, z is nuclear charge (# of protons), and n is integer (energy level)

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31
Q

Know how to calculate change in energy of an e- changing energy level in an H atom

A

Subtract original energy from final energy using equation for energy. A positive value indicates the system has gained energy.

32
Q

What is the equation for the wavelength of light that must be absorbed for a certain change in energy?

A

(hc)/(change in energy) where h is planks constant (6.62610^-34) and c is the speed of light (2.9979*10^8 m/s). CHANGE OF ENERGY MUST BE ABSOLUTE VALUE. If the system is losing energy, a photon is emitted. IF it is gaining, you say a photon was absorbed

33
Q

What are the 3 characteristics of light?

A

wavelength, frequency, and speed.

34
Q

long wavelength means what frequency and energy? Short wavelength means what frequency and energy?

A

low frequency and low energy. High frequency and high energy.

35
Q

equation relating wavelength, speed, and frequency?

A

wavelength*frequency = speed of light

36
Q

what is the SI unit for frequency?

A

1/s or a Hz

37
Q

Was the bohrs model successful for all atoms?

A

No, only applied to H, other atoms did not work. He did manage to show quantization of energy however.

38
Q

Who developed quantum mechanical model?

A

Werner Heisenberg, Louis de Broglie, and Erwin Schrodinger.

39
Q

What was the approach of quantum mechanical model?

A

viewed e- as a standing wave. Only certain orbits are shaped for e- to shape.

40
Q

What is an orbital?

A

it has a characteristic energy and shape. Wave function gives no detailed info about it

41
Q

Schrodingers EQ?

A

HY = EY

42
Q

Heisenberg uncertainty principle?

A

There is an uncertainty in simultaneously knowing both the position and momentum of an e- at a given time

43
Q

Quantum numbers

A

Each orbital is described by a series of numbers that describes various properties. You have principle quantum number (n), angular momentum quantum # (l), Magnetic quantum #(m1), and electron spin number (m2).

44
Q

All orbital shapes? How many e- can be held in each.

A

S, P, D, and F. 2, 6, 10, and 14. An orbital in each subshell holds 2.

45
Q

Pauli Exclusion Principle?

A

In a given atom, no 2 electrons can have same set of 4 quantum numbers (principle, angular momentum, magnetic, and electron spin) AN ORBITAL CAN ONLY HOLD 2 E- AND EACH HAS OPPOSITE SPINS DUE TO THIS!!! Many atoms have 2e- with 3 numbers the same, just not spin

46
Q

E- correlation problem

A

e- pathway cannot be known for atoms w/ more than one e-, so repulsion cannot be exactly calculated.

47
Q

Aufbaus principle?

A

Lower energy levels are filled first (4s is filled before 3d)

48
Q

Hunds rule?

A

Orbitals fill one at a time before pairing up

49
Q

Lathanides and Actinides

A

Lathanides: elements in which the 4f orbitals are filled. Sometimes 1-2 e- occupy the 5d orbital before 4f, since they have similar energy levels
Actinides: elements in which the 5f orbitals are filled. Sometimes 1-2 e- occupy the 5d orbital before 4f, since they have similar energy levels.

50
Q

What are the two electron configuration anomalies you have to know?

A

Cr and Cu (4s orbital is half filled)

51
Q

what did mendeleev do? What did moseley do?

A

correctly predicted elements to be discovered. Showed organizing table by atomic # showed better correlations

52
Q

Trend for ionization energy? why?

A

Decreases down a group (e- are further from nucleus). Increases down a period (because e- are being added and do not fully shield each other). Ionization energy also increases with each e- removed, and spikes whenever you start removing core e-

53
Q

Equation for effective nuclear charge?

A

Zeff = Z =S where Z is number of protons and S is number of shielding e-

54
Q

What anomalies do you have to know for ionization energy? Why does it happen?

A

decrease in Be to B, N->O. Orbitals begin to double in the P, causing e- repulsion.

55
Q

What is Electron affinity? What does it mean? What is the trend?

A

the energy change associated w/ addition of an e- to a gaseous atom. The more negative the electron affinity, the greater the tendency for an atom to accept an e-. A very negative EA means it is an exothermic process (lower energy), and lower energy is always better. A positive EA means the anion is higher in energy than the separated atom and e-. Increases across a period, and decreases down a group (generally).

56
Q

What are the anomalies for EA? What are the examples of stable and stable ions?

A

Fluorine is an anomaly for its group. It has a smaller EA than Cl , but the rest of the group follows the trend. This is due to the small 2p orbital.

N-> N- (unstable since e- repulsion in occupied orbital), C -> C- is stable, O -> O- is stable, and O- -> O2- is unstable, and reacts quickly to form oxide compounds

57
Q

How is Atomic Radius obtained for different compounds? Trends?

A

Covalent atomic radius: obtained from half of the distance between nonmetal atoms

Metallic radii: half the distance between the metal atom in a solid metal crystal

Non-metallic radii: atoms that do not form diatomic molecules are measured by estimating from various compounds

Decreases down a period due to increased Zeff and less shielding e-, and increases down a group since energy levels are bigger

58
Q

How does atomic radius change for ions?

A

A cation is smaller, and an anion is larger.

59
Q

What are isoelectric ions? How does their size compare?

A

Same number of e-. For these ions, size decreases when proton count increases. O2->F->Na+>Mg2+>Al3+

60
Q

What is photoelectron spectroscopy?

A

used to determine the energy of e- in an atom. High energy photons are directed at a sample and kinetic energy of released e- is measured.

61
Q

Ionic bonds?

A

between metal and nonmetal

62
Q

What is lattice energy? How can it be determined? Equation for it? Trend for lattice energy?

A

The energy required to separate a mole of ionic compound into gaseous ions. It can be derived theoretically or from a thermodynamic cycling reaction: the born Haber cycle. Eel = (KQ1Q2)/d^2. K = 8.99*10^9, Q1 and Q2 are the charges on the particles, and d is distance. It calculates attraction force in JOULES. Formation of a lattice is an exothermic process. Lattice energy increases as charge increases, or when radii decreases!!! Ex: NaCl has a larger intramolecular force than CsI due to smaller atomic radius. CaO has a higher lattice energy than KI due to larger chargers

63
Q

What is electronegativity?

A

tendency for an atom to pull shared e- to itself

64
Q

Trends for Electronegativity?

A

increases down a period, decreases down a group. Same as Ionization energy.

65
Q

Most electronegative element? Least?

A

Fluorine. francium and Cesium.

66
Q

what is a polar covalent bond? What causes it?

A

Where there are partial charges on the molecule due to one atom being more electronegative than the other.

67
Q

Who developed a scale for electronegativity?

A

Linus Pauling

68
Q

How to calculate difference in electronegativity? What determines if they are ionic, polar, or nonpolar?

A

Subtract larger value from less. If it is 2 or more, it is likely ionic. If it is between 0.4-1.9 it is likely polar. If it is less than 0.4 it is likely nonpolar.

69
Q

Know how to draw lewis structures

A
70
Q

Octet rule?

A

Metals and nonmetals tend to form the most stable molecules when they are surrounded by 8e-

71
Q

Exceptions to octet rule?

A

Be (most stable w 4e-) and B (stable w 6e-). 3rd period and beyond can house more than 8

72
Q

What are dipoles? What is dipole moment?

A

They have a positive center and a negative center. dipole moment: a property of a molecule whose charge distribution can be represented by a center of + charge and a center of - charge.

73
Q

Why can some molecules have polar bonds, but no dipole moment?

A

The bonds are arranged in a way that cancels out charges. Polarity is also dependent on shape.

74
Q

What three shapes can be polar but have no dipole moment?

A

linear (180), trigonal planar (120), and tetrahedral (109.5).

75
Q

Types of calculations you have to know: stoichiometry, calculate empirical formula from chemical analysis, % mass composition, empirical to molecular formula

A
76
Q

know polyatomic ions

A

Chemistry (6 decks)

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