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KME Chemistry > 3 Sem, 2 Exam > Flashcards

3 Sem, 2 Exam Flashcards

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1
Q

How did Bohr label the shells of an atom?

A

K, L, M etc. or 1, 2, 3 etc.

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2
Q

Number of possible electrons on a shell?

A

2n^2

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3
Q

Who came up with the quantum-mechanical calculations that from the modern atomic model?

A

Erwin Schrödinger and Werner Heisenberg

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4
Q

What are the four types of atomic orbitals (in order) and how many electrons can they hold?

A

s: sharp (2), p: principal (6), d: diffuse (10), f: fundamental (14)

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5
Q

How is the first atomic shell built up?

A

Is built up of one subshell which is built up of one s orbital.

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6
Q

How is the second atomic shell built up?

A

The second shell has two subshells. One has one s orbital in it, so a total of 2 electrons, and the other has 3 p orbitals in it, for a total of 6. That means altogether the second shell can contain 8 electrons.

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7
Q

What should one be careful of when writing electron configurations in the d and f block?

A

That the d orbitals are in the previous shell and must be written as “shell#-1” and the f orbitals as “shell#-2”

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8
Q

What does the solution of the Schrödinger equation give?

A

The energy content of the orbitals (E).

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9
Q

How many different orbitals are there in the subshells?

Give the shape to the first two.

A

s=1 (sphere), p=3 (dumbbell shaped orthogonal along x, y and z axes), d=5, f=7

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10
Q

Who discovered the electron spin?

A

Wolfgang Pauli

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11
Q

What two factors describe the status of an electron in an atom?

A

Its orbital and its spin (up-spin and down-spin)

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12
Q

How does one “fill-in” the spins of electrons?

A

The number of electrons is given by the element and its corresponding atomic number. The subshells are filled with electron (from the bottom up on an energy scale). Each subshell is filled giving each orbital an up-spin, when all the orbitals of a subshell are filled with electrons (from left to right) they are filled with down-spins (a.k.a. second electrons).

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13
Q

Who is responsible for the first concept of the periodic table?

A

Dmitri Iwanowitsch Mendelejew and Lothar Meyer

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14
Q

What does the ionization energy measure?

A

The ionization energy measures the energy that is required to remove one electron from an atom in its gaseous state. This process is called ionization

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15
Q

Which elements have the highest ionization energies?

A

The elements with completely occupied p-orbitals (He, Ne, Ar, etc.). The noble gasses + He.

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16
Q

What are the rows (a) and the columns (b) of the periodic table called?

A

a) periods

b) groups

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17
Q

What are the (a) leftmost, (b) second leftmost, (c) all d-block, (d) all f-block, (e) second rightmost and (f) rightmost elements on the periodic table called?

A

a) Alkali metals
b) Alkali earth metals
c) d-transition metals / transition group / transition elements / transition metals
d) f-transition metals / inner transition elements (4f-line: lanthanides, 5f-line: actinides)
e) Halogens
f) Noble gases

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18
Q

Properties of alkali metals?

A

Very soft, extremely reactive (need to be stored in paraffine), reactions with water produce alkaline solutions, float in water (density: alk. metals < H2O)

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19
Q

What is a valence electron and how else is it called?

A

A valance electron or outer electron is an electron on the outermost shell of an atom, that can participate in the formation of a chemical bond.

20
Q

a) Why do elements in the same group have a similar reactive behavior?
b) Do some elements deviate from their group’s behavior and because of which factor?

A

a) Because they have the same amounts of valence electrons.

b) Yes, because of the metallic character.

21
Q

How does the the metallic character of the elements show itself on the periodic table?

A

The metallic properties decrease from left to right and increase from top to bottom, except for Hydrogen, which is a non metal.

22
Q

The occupation of the orbitals with the electrons and their spins?

A

Hund’s Rule

23
Q

What else is the octet-rule called and what does it signify?

A

The octet- or noble gas rule is that atoms are always seeking the state in which they have eight valence electrons in their outermost shell.

24
Q

Who devised the method in which one can represent covalent bonds in a simple manner and what is this theory called?

A

G.N. Lewis discovered the Lewis Formula.

25
Q

What is the bare atom (without valence electrons) called in the Lewis Formula?

A

Torso

26
Q

How do you know how many valence electrons to draw in the Lewis Formula?

A

Count from left to right on the periodic table from the beginning of the row (a new shell is filled up with electrons from the left).

27
Q

How do atoms try to fulfill the noble gas rule?

A

Atoms form covalent or atomic bonds, in which they share valence electrons with each other to form a molecule.

28
Q
  1. Draw the formation of F2 from two fluorine atoms.
  2. Draw the formation of O2 from two oxygen atoms.
  3. Draw the formation of N2 from two nitrogen atoms.
  4. Draw the formation of C2 from two carbon atoms.
    (Use the Lewis formula to show these bonds)
A

page 40

29
Q

In what forms does pure carbon occur in nature and what are these “forms” called?

A

Carbon exists in three allotropes:

diamond, graphite, buckminsterfullerens/buckyballs

30
Q

What are the build, properties and uses of diamonds?

A

a) Regularly arranged atoms in a lattice structure, each atom is surrounded by four other C-atoms in a tetrahedral form
b) Colorless, dispersive, hardest known mineral, electrical isolator
c) Jewelry, industrial applications (drilling)

31
Q

What are the build, properties and uses of graphite?

A

a) One-atom-thick layers of carbon atoms stacked on top of each other, the C-atoms in the layers form hexagons
b) Black, shiny, soft, electrically conductive
c) Electrodes, grease/lubricant, pencils

32
Q

What are the build and uses of buckminsterfullerens?

A

a) Carbon atoms form a cage like structure connected in hexagons and pentagons, the formula is (C60 or C70)
b) nanotechnology, semiconductors

33
Q

Why is a diamond so strong?

Why is a diamond an electrical isolator?

A

a) Regular arrangement (…) and the strong covalent bonds which keep C-atoms in their positions.
b) Because there are no free electrons in the diamond lattice

34
Q

How is graphite a graphite hexagon built up?
What is its outcome (phenomenon)?
Give the reason for graphite’s electrical conductivity.
Use and define the necessary words.

A

Within one layer every C-atom is bound to three other C-atoms. The delocalized electron is the fourth valence electron of the carbon atoms. Six such delocalized electrons form three bonds in each hexagon. The fact that the positions of the bonds are not determinable leads to the phenomenon of resonance and is the reason graphite is electrically conductive.

35
Q

Why are is graphite so soft?

A

Because there are only small forces holding the single layers together which makes the layers slidable and the graphite soft.

36
Q

What is a resonant state?

A

In a hexagonal or pentagonal carbon lattice, the double bonds jump around and the position of single and double bonds change.

37
Q

Define molecules.

A

Small, finite and defined collectives of nonmetal atoms, which are connected by covalent bonds.

38
Q

Define compounds.

A

Atomic collectives which consist of atoms with different number of protons. These can be metal and non-metal.

39
Q

Define bonds and give two examples.

A

Forces that act between atoms. Covalent bonds (molecules) and ionic bonds (salts).

40
Q

Atoms connecting to a central one of a compound?

A

Ligand

41
Q

Draw and label a 3D molecule in 2D.

A

page 43

42
Q

What does VSEPR-Model stand for?

A

Valence Shell Electron Pair Repulsion

43
Q

Why are the hydrogen atoms pushed down in a water molecule?

A

Because lone electrons have a stronger repulsion towards other electrons than shared electrons.
Or
The four non bonded electrons on the Oxygen atom bind themselves together and the atom becomes an atom with bonds 4 directions so the shape becomes tetrahedral.

44
Q

What are the binding properties of (a) Hydrogen, (b) Halogens, (c) Oxygen and (d) Nitrogen?

A

a) always one bond
b) usually one bond
c) always two bonds
d) usually three bonds

45
Q

What is the shape and angle of a molecule with (a) 2, (b) 3, (c) 4, (d) 5 or (e) 6 charge centers, or electron pairs/bonds in the x direction? (angle only for firs three)

A

a) linear, 180°
b) trigonal, planar, 120°
c) tetrahedral, spatial, 109.5°
d) trigonal, bipyramidal
e) octahedral

46
Q

Projection formula for H2CO, C2H4, C2H2, HCN and CO2?

A

page 44

KME Chemistry (5 decks)

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