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Chemistry Module 2 - Own Flashcards > Chapter 2 - Atoms, Ions and Compounds > Flashcards

Chapter 2 - Atoms, Ions and Compounds Flashcards

1
Q

What are the three subatomic particles found in the atom? Where are each of these found?

A
  1. Atoms consist of a nucleus, made up of protons and neutron
  2. Electron occupy the region of space around the nucleus and are arranged in shells.
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2
Q

Instead of grams, what do chemists use to measure the masses of subatomic particles?

A

Atoms and their subatomic particles have tiny masses instead of working in grams chemists compare the masses of subatomic particles using relative masses

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3
Q

What abbreviation is used to represent protons?

A

p+

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4
Q

What abbreviation is used to represent neutrons?

A

n

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5
Q

What abbreviation is used to represent electrons?

A

e-

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6
Q

What is the relative charge of a proton?

A

1+

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7
Q

What is the relative charge of a neutrons?

A

0

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8
Q

What is the relative charge of an electron?

A

1-

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9
Q

What is the relative mass of a proton?

A

1

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10
Q

What is the relative mass of a neutron?

A

1

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11
Q

What is the relative mass of an electron?

A

1/1836

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12
Q

Where is most of the atom’s mass located?

A

The nucleus

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13
Q

What is known about the number of protons and electrons in an atom? What does this result in?

A

Atoms contain the same number pf protons as electrons.

The total positive charge from protons is cancelled by the total negative charge from electrons.

The overall charge of an atom is zero - an atom is neutral.

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14
Q

What role do neutrons play in the nucleus of an atom?

A

Neutrons act as the glue that holds the nucleus together, countering the electrostatic repulsion between the positively charged protons.

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15
Q

How does the number of neutrons compare to the number of protons in most atoms?

A

Most atoms contain the same number of, or slightly more, neutrons than protons.

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16
Q

What happens to the number of neutrons required as the nucleus gets larger?

A

As the nucleus gets larger, more and more neutrons are needed to stabilize it.

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17
Q

What is the atomic number of an element?

A

The atomic number is the identity of an element, indicating the number of protons in an atom of that element.

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18
Q

How does the number of protons in an atom relate to its identity?

A

The number of protons identifies the element; every atom of the same element contains the same number of protons.

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19
Q

What distinguishes atoms of different elements?

A

Different elements contain atoms with different numbers of protons.

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20
Q

As of 2014, how many elements have been confirmed?

A

114 elements have been confirmed, with others tentatively reported.

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20
Q

How are elements arranged in the periodic table?

A

Elements are arranged in order of their number of protons (atomic number), with each element shown alongside its atomic number.

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21
Q

What is the atomic number of hydrogen (H)?

A

1

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22
Q

What is the atomic number of helium (He)?

A

2

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23
Q

What is the atomic number of lithium (Li)?

A

3

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24
Q

What is the atomic number of beryllium (Be)?

A

4

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25
Q

What is the atomic number of boron (B)?

A

5

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26
Q

What is the atomic number of carbon (C)?

A

6

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27
Q

What is the atomic number of nitrogen (N)?

A

7

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28
Q

What is the atomic number of oxygen (O)?

A

8

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29
Q

What is the atomic number of fluorine (F)?

A

9

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30
Q

What is the atomic number of neon (Ne)?

A

10

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31
Q

What is the atomic number of sodium (Na)?

A

11

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32
Q

What is the atomic number of magnesium (Mg)?

A

12

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33
Q

What is the atomic number of aluminum (Al)?

A

13

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34
Q

What is the atomic number of silicon (Si)?

A

14

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35
Q

What is the atomic number of phosphorus (P)?

A

15

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36
Q

What is the atomic number of sulfur (S)?

A

16

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37
Q

What is the atomic number of chlorine (Cl)?

A

17

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38
Q

What is the atomic number of argon (Ar)?

A

18

39
Q

What is an isotope?

A

Isotopes are atoms of the same element with different numbers of neutrons and different masses.

40
Q

What remains the same in every atom of a given element?

A

The number of protons is the same in every atom of a given element.

41
Q

Are most elements composed of a single isotope or a mixture of isotopes?

A

Most elements are made up of a mixture of isotopes.

42
Q

What is the mass number (A), and how is it calculated?

A

The mass number (A) is the total number of protons and neutrons in an atom, calculated as:
A = numberofprotons + numberofneutrons

43
Q

What is the atomic number (Z), and what does it represent?

A

The atomic number (Z) represents the number of protons in an atom.

44
Q

How do you determine the number of protons, neutrons, and electrons in an isotope from its chemical notation?

A
  1. Protons = Atomic number (Z)
  2. Neutrons = Mass number (A) - Atomic number (Z)
  3. Electrons = Number of protons (in a neutral atom).
45
Q

Why do isotopes of the same element behave identically in chemical reactions?

A

Chemical reactions involve the electrons, and all isotopes of an element have the same number of electrons.

46
Q

Does the number of neutrons affect the chemical reactivity of isotopes?

A

No, the number of neutrons does not affect the chemical reactivity of isotopes.

47
Q

What physical properties might differ between isotopes of the same element?

A

Higher-mass isotopes may have higher melting points, boiling points, and densities.

48
Q

What is an ion?

A

An ion is a charged atom where the number of electrons differs from the number of protons.

49
Q

What are cations?

A

Cations are positively charged ions with fewer electrons than protons.

50
Q

What are anions?

A

Anions are negatively charged ions with more electrons than protons.

51
Q

What type of charge does a cation have?

A

Cations have an overall positive charge.

52
Q

What type of charge does an anion have?

A

Anions have an overall negative charge.

53
Q

How are ions shown in relation to their charge?

A

Ions are shown with their overall relative charge, such as Mg2+ and Cl-

54
Q

How does Mg2+ differ in terms of electrons and protons?

A

Mg2+ has two fewer electrons than protons.

55
Q

How does Cl- differ in terms of electrons and protons?

A

Cl- has one more electron than protons.

56
Q

What is the number of protons, neutrons, and electrons in 24,12, Mg2+?

A

Protons: 12
Neutrons: 12
Electrons: 10

57
Q

What is the overall charge of 24,12, Mg2+?

A

2+
BECAUSE:
12 protons = 12+
10 electrons = 10-
Net charge = 12-10 = 2

58
Q

What is the number of protons, neutrons, and electrons in 35,17,Cl-?

A

Protons: 17
Neutrons: 18
Electrons: 18

59
Q

What is the overall charge of 35,17,Cl-?

A

1-
BECAUSE:
17 protons = 17+
18 electrons = 18-
Net charge = 17-18 = -1

60
Q

How do ions and atoms of an element differ in terms of protons and electrons?

A

Ions and atoms of an element have the same number of protons but a different number of electrons.

61
Q

What is relative isotopic mass?

A

The relative isotopic mass is the mass of an isotope relative to 1/12th of the mass of an atom of carbon-12.

62
Q

Why does relative isotopic mass have no units?

A

Because it is a ratio of two masses.

63
Q

Give examples of relative isotopic masses for common isotopes:

A

12,C = 12.0
14,N = 14.0
16,O = 16.0

64
Q

What is relative atomic mass?

A

Relative atomic mass is the weighted mean mass of an atom of an element relative to 1/12th of the mass of an atom of carbon-12.

65
Q

What two factors does the weighted mean take into account?

A
  1. The percentage abundance of each isotope.
  2. The relative isotopic mass of each isotope.
66
Q

How is relative atomic mass represented in the periodic table?

A

It is shown underneath the atomic number, such as 28.1 for silicon or 31.0 for phosphorus.

67
Q

What is the principle of a mass spectrometer?

A
  1. A sample is placed in the mass spectrometer.
  2. The sample is vaporized and ionized to form positive ions.
  3. The ions are accelerated. Heavier ions move more slowly and are more difficult to deflect than lighter ions, so they separate by mass.
  4. The ions are detected on a mass spectrum as a mass-to-charge ratio (m/z)
68
Q

What does the height of each peak on a mass spectrum represent?

A

The percentage abundance of the isotope.

69
Q

How is the relative atomic mass calculated from a mass spectrum?

A

(sum of (isotope mass x isotope abundance)) ÷ total isotopes abundance

70
Q

How do you calculate the relative atomic mass of chlorine using isotopes?

A

(Abundanceof
35,Cl×Massof 35,Cl)+(Abundanceof
37,Cl×Massof37,Cl) ÷ 100

71
Q

What type of ions do metals form, and how?

A

Metals lose electrons to form cations (positive ions).

72
Q

What type of ions do non-metals form, and how?

A

Non-metals gain electrons to form anions (negative ions).

73
Q

What are the charges for ions in periodic table groups?

A

Group 1: +1
Group 2: +2
Group 5: -3
Group 6: -2
Group 7: -1
Group 0 (noble gases): Neutral (0)

74
Q

Give examples of transition metals that form ions with different charges.

A

Copper:
1. Copper(I) = Cu+
2. Copper(II) = Cu2+

Iron:
1. Iron(II) = Fe2+
2. Iron(III) = Fe3+

75
Q

What is a binary compound? Give an example.

A

A compound containing only two elements. Example: Sodium oxide (Na2O).

76
Q

How do you name binary compounds?

A

Name the first element, then change the ending of the second element to “-ide.”

77
Q

What are polyatomic ions?

A

Ions that contain atoms of more than one element bonded together.

78
Q

List all 11 polyatomic ions (names only.)

A
  1. Ammonium
  2. Hydroxide
  3. Nitrate
  4. Nitrite
  5. Hydrogencarbonate
  6. Manganate(VII)
  7. Carbonate
  8. Sulphate
  9. Sulphite
  10. Dichromate(VI)
  11. Phosphate
79
Q

What is the chemical formula and charge of ammonium?

A

Formula: (NH4(+))
Charge: 1+

80
Q

What is the chemical formula and charge of hydroxide?

A

Formula: (OH(-))
Charge: 1-

81
Q

What is the chemical formula and charge of nitrate?

A

Formula: (NO3(-))
Charge: 1-

82
Q

What is the chemical formula and charge of nitrite?

A

Formula: (NO2(-))
Charge: 1-

83
Q

What is the chemical formula and charge of hydrogencarbonate?

A

Formula: (HCO3(-))
Charge: 1-

84
Q

What is the chemical formula and charge of Manganate(VII) (permanganate)?

A

Formula: (MnO4(-))
Charge: 1-

85
Q

What is the chemical formula and charge of carbonate?

A

Formula: (CO3(2-))
Charge: 2-

86
Q

What is the chemical formula and charge of sulfate?

A

Formula: (SO4(2-))
Charge: 2-

87
Q

What is the chemical formula and charge of sulphite?

A

Formula: (SO3(2-))
Charge: 2-

88
Q

What is the chemical formula and charge of Dichromate(VI)?

A

Formula: (Cr2O7(2-))
Charge: 2-

89
Q

What is the chemical formula and charge of Phosphate?

A

Formula: (PO4(3-))
Charge: 3-

90
Q

What are the key rules for writing ionic formulas?

A
  1. Total positive charges = Total negative charges (neutral overall).
  2. Use subscripts to show the number of ions.
  3. Use brackets for multiple polyatomic ions.
91
Q

What is the formula of aluminum sulfate?

A

Al2(SO4)3

92
Q

How are elements represented in chemical equations?

A
  1. Elements are shown as symbols.
  2. Diatomic molecules: H2, N2, O2, F2, Cl2, Br2, and I2
  3. Exceptions: P4 (Phosphorous) and S8 (Sulfure)
93
Q

What are state symbols in equations?

A

(g) = gas
(l) = liquid
(s) = solid
(aq) = dissolved in water otherwise known as aqueous

94
Q

How do you balance an equation?

A
  1. Adjust balancing numbers (in front of formulas).
  2. Ensure the number of atoms of each element is the same on both sides.
  3. Do not alter chemical formulas.
95
Q

How do you balance equations with brackets?

A

The balancing number multiplies the entire formula, including the contents inside brackets.

Chemistry Module 2 - Own Flashcards (10 decks)

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