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Inorganic Chemistry > Unit 2 > Flashcards

Unit 2 Flashcards

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1
Q

What did Zeno of Elea (~450 BCE) believe?

A

Did not believe in atoms. Believed matter was divisible and you could not reach a point in which a particle of matter was not divisible. (Infinitely divisible)

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2
Q

What did Democritus (~460-370 BCE) believe?

A

Matter is made of very small indestructible units called atoms.

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3
Q

Who was correct in their theory of atoms: Zeno or Democritus?

A

Democritus because atoms are the basic unit of matter.

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4
Q

What is an element?

A

A substance that consists of the same kind of atoms.

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5
Q

What are the 6 essential elements of living organisms?

A

Carbon, hydrogen, nitrogen, oxygen, phosphorus, and sulfur.

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6
Q

What is a compound?

A

A substance with a fixed ratio of mass of elements. It is characterized by its chemical formula.

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7
Q

About how many compounds are known?

A

~20 million

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8
Q

What is a compound formula?

A

A formula that indicates the atomic symbol of each element and subscript indicates the ratio of elements.

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9
Q

What is Daltons theory?

A

Was the foundation of modern atomic theory (1808). Had evidence to substantiate Democritus’ theory.

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10
Q

How many postulates are in Daltons Atomic Theory?

A

5 postulates

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11
Q

What is the 1st postulate in Daltons theory?

A

All matter is made up of very tiny, indivisible particles called atoms.

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12
Q

What is the 2nd postulate in Daltons theory

A

All atoms of a given element have the same chemical properties and atoms of different elements have different chemical properties.

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13
Q

What is the 3rd postulate in Daltons theory

A

In ordinary chemical reactions, no atoms of any element can disappear or change into an atom of a different element.

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14
Q

What is the 4th postulate in Daltons theory

A

Compounds are formed by the chemical combination of two or more different kinds of atoms. In a compound, the relative numbers of each kind of element are consistent.

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15
Q

What is the 5th postulate in Daltons theory

A

A molecule is a tightly bound combination of two or more atoms that acts as a single unit.

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16
Q

How does the Law of Conservation of Mass support Daltons theory?

A

The total mass of matter at the beginning and the end of an ordinary chemical reaction is the same. Matter can neither be created or destroyed.

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17
Q

How does the Law of Constant Composition support Daltons theory?

A

Any compound is always made up of elements in the proportion of mass.

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18
Q

What is a monoatomic element?

A

Consists of single atoms that are not connected to each other.

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19
Q

What is a diatomic element?

A

Two atoms in each molecule are connected by a chemical bond. Under normal conditions, free atoms don’t exist for these atoms.

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20
Q

What is a polyatomic element?

A

More than 2 atoms in each molecule, connected by chemical bonds.

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21
Q

What is the composition of an atom?

A

Composed of 3 subatomic particles called protons, neutrons, and electrons.

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22
Q

What makes up the nucleus of an atom?

A

Protons and neutrons

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23
Q

Where do electrons fit in an atom?

A

Some protons and neutrons are charged, which will have electrons around the nucleus. Creates an “electron cloud.”

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24
Q

What is Mass Number (A)?

A

Is a way to describe an atom. Used to express the relative masses of elements in a compound.

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25
Q

How is mass number found?

A

of protons + # of neutrons = mass

26
Q

What is atomic number (Z)?

A

Number of protons in the nucleus. All atoms of the same element have the same number of protons.

27
Q

How many atomic numbers are there? (How many elements)

A

118 elements = 118 atomic numbers (Z)
Neutral atoms: # e- = # p+

28
Q

Isotopes of an element have the same atomic number but a different atomic mass. True of False?

A

True

29
Q

Isotopes tend to have the same properties other than what?

A

Radioactivity

30
Q

Atomic weight shows relative atomic mass based on what?

A

Weighted sum of all the isotope masses.

31
Q

What is an isotope?

A

Atoms within an element that have the same number of protons but different number of neutrons.

32
Q

Do isotopes of an element have the same atomic number (Z) and atomic mass (A)?

A

No, isotopes have the same atomic number but different atomic mass.

33
Q

Do most elements found on earth have mixtures of isotopes in relative ratios and why is this important?

A

Yes, it is important when wanting to differentiate between atomic mass and atomic weight.

34
Q

What does atomic mass number (A) refer to? And, how is this found?

A

The mass of a specific isotope and is found by adding the mass of protons and neutrons.

35
Q

What is atomic weight?

A

The weighted average of masses of all isotopes for a given element.

36
Q

(Isotopic mass x natural abundance (%))/total abundance of element (100%) is the formula for what?

A

Atomic Weight

37
Q

Where is the mass of an atom concentrated?

A

In the nucleus

38
Q

In neutral atoms, are electrons the same amount of protons?

A

Yes

39
Q

What was Niels Bohr theorize?

A

Electron energy is quantifiable

40
Q

Do electrons move freely around nucleus?

A

No, they are confined to specific regions. Think “shells”

41
Q

How are electron shells numbered?

A

Numbered inside to out. 1, 2, 3, etc., and each can only hold a specific amount of electrons.

42
Q

How many electrons can each level hold?

A

1st = 2
2nd = 8
3rd = 18
4th = 32

43
Q

Can an electron move from one level to another?

A

Yes, but only if the energy it gains or loses is exactly equal to the difference in energy between the two levels.

44
Q

What is the 1st and 2nd step to drawing orbitals and electrons?

A

First, find the number of electrons in the element. Second, assign the number of shells to the electrons.

45
Q

What is the third and final step to drawing orbitals and electrons?

A

Draw the orbit and place the electrons in their respective shells, without exceeding the capacity of each shell.

46
Q

What is a valence electron?

A

Electrons in the outermost (valaemce shell) of an atom.

47
Q

What is the Lewis dot structure?

A

A way to represent the valence electrons of an atom with dots around the chemical symbol.

48
Q

What is atomic size and how is it determined?

A

The diameter of an atom. It is determined by the size of its outermost occupied orbital.

49
Q

How is the atomic radius found?

A

Atomic size divided by 2

50
Q

How does atomic radius work within the periodic table?

A

Atomic radii (ironic radius) of elements increases as you progress down the groups (columns).

51
Q

Explain what happens involving the ionic radius as you go down a group.

A

Ionic radius increases, more shells of electrons. Also, less attraction means electrons are pulled in less by the nucleus.

52
Q

Do atomic radii increase or decrease to the left across the periods (rows)?

A

They increase because more protons in the nucleus results in higher nuclear charge. This pulls the e- closer to the nucleus.

53
Q

Are atoms electrically neutral?

A

Yes, #p = # e-

54
Q

Can atoms gain/lose electrons?

A

Yes

55
Q

Explain “ion” and the 2 types.

A

Ian is an atom with unequal # of protons and electrons. Anion is an ion with a - charge. Cation is an ion with a +charge.

56
Q

When do cations form?

A

When electrons are removed from an atom.

57
Q

When do anions form?

A

When an atom gains eelectrons.

58
Q

What is ionization energy and what property is it?

A

It is a physical property if elements. It is the energy required to remove the most loosely held electron from an atom in the gaseous phase.

59
Q

Is it easier or more difficult to remove an electron with a higher ionization energy?

A

It is more difficult to remove an electron. Ionization energy is always positive. Energy must be supplied to remove attractive force between the nucleus and electrons.

60
Q

Explain how ionization energy increases as you go up a column (bottom to top).

A

Electrons further from the nucleus are shielded by inner electrons and less attracted to the nucleus. Therefore, less IE is required to remove the outermost electron(s).

61
Q

Explain how ionization energy increases as you go across a row (left to right).

A

Valence electrons across a row are in the same shell, but the bumper of protons in the nucleus increase (Z), which increases outer e- attraction to the nucleus and makes them harder to remove.

Inorganic Chemistry (3 decks)

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