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Chemistry and Our Universe > Chapters 7-12 > Flashcards

Chapters 7-12 Flashcards

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1
Q

How do atoms of phosphorus and Sulfur tend to appear in nature?

A

As bonded groups of 4 (P) and 8 (S) atoms.

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2
Q

What is a sigma covalent bond?

A

Sigma bonds are the result of orbital overlap directly
between the 2 bonded nuclei on the internuclear axis. These kinds of bonds can form when either an s orbital or p orbital overlap.

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3
Q

What are covalent bonds?

A

Bonds in which electrons are shared between two elements, not transferred.

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4
Q

What formula produces a square planar molecular

A

AX4E2

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5
Q

What is an empirical formula?

A

A formula that simply provides the ratios of the constituent elements in a compound.

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6
Q

What kind of molecular geometry do diatomic molecules have?

A

The only kind they can, a straight line.

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7
Q

What formula produces a tetrahedral molecular geometry?

A

AX4E0

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8
Q

What kind of molecular geometry does the formula AX2E0 have?

A

Linear. C02 is an example.

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9
Q

Who was the first to determine the weight of a molecule? When?

A

Jean-Baptiste Dumas, 1826.

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10
Q

What does each new row in the periodic table represent?

A

The first electron to populate a new principal energy level.

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11
Q

What is a molecular formula?

A

A formula that provides the exact number of atoms of each element in a molecule of a particular element.

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12
Q

What formula produces a trigonal bipyramidal molecular geometry?

A

AX5E0

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13
Q

What are Gilbert Lewis’s dates?

A

1875-1946.

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14
Q

Where do we find regions of high electron density in the valence shell of an atom?

A

In the orbitals holding lone pairs and in orbitals forming bonds to other atoms.

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15
Q

What is an electron domain?

A

a concerted region of electron density in the valence shell of an atom.

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16
Q

What is the name of the theory that describes the 3-dimensional structures of molecules?

A

Valence Shell Electron Pair Repulsion (VSEPR) theory.

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17
Q

What is a shortcoming of the molecular formula of molecules?

A

It doesn’t indicate how those atoms are arranged in space.

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18
Q

What formula produces a trigonal pyramidal molecular geometry?

A

AX3E1

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19
Q

What kind of molecular geometry does the formula AX4E1 have?

A

See-saw. SF4 is an example.

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20
Q

How does electronegativity trend on the periodic table?

A

The reverse of the first ionization energy, elements like fluorine having the greatest electronegativity and elements like cesium and francium having the smallest.

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21
Q

What formula produces a T-shaped molecular geometry?

A

AX3E2

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22
Q

What makes elements with similar properties similar?

A

The configuration of their valence electron shells.

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23
Q

What is the Pauling Scale?

A

The scale the measures electronegativity on a scale from 0 to 4, with 4 being fluorine.

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24
Q

What is the trend in the radius of the atom as it moves across rows?

A

Decreasing atomic radius as we move left to right; Increasing as we move right to left.

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25
Q

What formula produces a square pyramidal molecular

A

AX5E1

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26
Q

What kind of molecular geometry does the formula AX2E1 have?

A

Bent. O3 is an example.

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27
Q

What kind of molecular geometry does the formula AX2E2 have?

A

Bent. H2O is an example.

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28
Q

What counterbalances the size growth do to more and more electron shells?

A

The electrostatic attraction to the increasingly positive nucleus as more protons are added.

29
Q

What formula produces a octahedral molecular

A

AX6E0

30
Q

What is electronegativity?

A

It is the flip side of first ionization energy and refers to how easily a neutral atom picks up an electron.

31
Q

What is the trend in the radius of the atom as it moves up or down a column?

A

Radius decreases as we move up a column; increases as we move down a column.

32
Q

What kind of molecular geometry does the formula AX3E0 have?

A

Trigonal Planar. BF3 is an example.

33
Q

What are polar covalent bonds?

A

Ones in which the shared electrons spend a bit more time around one element than the other, causing the system to have polarity.

34
Q

What is the force that causes atoms to “want” to overcome electrostatic forces and get close to one another?

A

The powerful tendency of atoms to form valence octets.

35
Q

What are the two types of covalent bonds that can form?

A

sigma bonds and pi bonds.

36
Q

What is first ionization energy?

A

The amount of energy needed to remove an electron from an atom and create a cation with a +1 charge.

37
Q

What important concept does VSEPR theory rest on?

A

The concept of electron domains.

38
Q

What is it about water that allows it to dissolve a variety of salts that form ions in solution?

A

The polar covalent oxygen‑hydrogen bonds in water each have a partial charge separation. And the fact that water is an AX2E2 molecule means that it has a bent geometry.

39
Q

How did Mendeleev choose columns for the periodic table?

A

By similar properties of the elements.

40
Q

What kind of molecular geometry does the formula AX6E0 have?

A

octahedral. SF6 is an example.

41
Q

What are Lewis structures?

A

Writing the symbol for the element with dots around it, representing the valence electrons.

42
Q

What is a good definition of a chemical bond?

A

An energetically beneficial interaction between atoms that confines them to a fixed distance from one another in space.

43
Q

What are some neutral atoms found in nature?

A

Argon in the atmosphere and gold in the earth.

44
Q

What formula produces a trigonal planar molecular geometry?

A

AX3E0

45
Q

What are Linus Pauling’s dates?

A

1901-1994.

46
Q

What kind of molecular geometry does the formula AX4E0 have?

A

tetrahedral. CH4 is an example.

47
Q

How does first ionization energy trend on the periodic table?

A

It increases as we move up and to the right on the table.

48
Q

What are ionic bonds?

A

Bonds in which 2 atoms that have a tendency to form ions of opposite charge exchange electrons to form valence octets.

49
Q

How much volume is occupied by one mole of gas at 1 atmosphere pressure and 0 degrees Celsius?

A

22.4 liters.

50
Q

What are the 3 major types of chemical bonds?

A

ionic bonds and covalent bonds make up the extremes, and polar covalent bonds fill in the gray areas between them.

51
Q

What kind of molecular geometry does the formula AX3E2 have?

A

T-shaped. ClF3 is an example.

52
Q

What is a cation?

A

An atom that has lost one or more electrons, resulting in a net positive charge.

53
Q

What formula produces a bent molecular geometry?

A

AX2E1 and AX2E2

54
Q

What is an anion?

A

An atom that has gained one or more electrons, resulting in a net negative charge.

55
Q

What is the allotrope of oxygen we encounter most commonly at the Earth’s surface?

A

Diatomic oxygen, two oxygen atoms joined by a double bond.

56
Q

What is the order of covalent bonding?

A

First bond is always sigma, additional bonds are always pi.

57
Q

What kind of molecular geometry does the formula AX3E1 have?

A

trigonal pyramidal. NH3 is an example.

58
Q

What kind of molecular geometry does the formula AX5E1 have?

A

square pyramidal. BrF5 is an example.

59
Q

What are cesium’s size properties in comparison to hydrogen?

A

Cesium has 133 times the mass of hydrogen but only 10 times the radius.

60
Q

What is the basic idea behind Linus Pauling’s theory of orbital hybridization?

A

when an atom bonds, its valence orbitals can combine and average out to form any number of identical orbitals needed for bonding.

61
Q

What kind of molecular geometry does the formula AX4E2 have?

A

square planar. XeF4 is an example.

62
Q

How do atoms of Oxygen and Nitrogen tend to appear in nature?

A

As diatomic molecules.

63
Q

What types of elements tend to form covalent bonds?

A

Ones with similar electronegativities.

64
Q

What is a typical distance between two bonded atoms?

A

An angstrom or two.

65
Q

What kind of molecular geometry does the formula AX5E0 have?

A

trigonal bipyramidal. PF5 is an example.

66
Q

How would researchers like Lavoisier and Faraday discover the empirical formulae of compounds?

A

By combustion analysis: burning the compound in excess oxygen and measuring the results.

67
Q

What formula produces a linear molecular geometry?

A

AX2E0

68
Q

What formula produces a see-saw molecular geometry?

A

AX4E1

69
Q

What are pi bonds?

A

The side‑on overlap of 2 sets of p orbitals can create a

shared space that holds 2 more sets of bonding electrons.

Chemistry and Our Universe (6 decks)

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