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online notes Flashcards

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1
Q

What is the atomic number related to?

A

Number of protons

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2
Q

What does the mass number represent?

A

Number of protons and neutrons

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3
Q

What characterizes a neutral atom?

A

Equal number of protons and neutrons

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4
Q

What is an anion?

A

An ion with more electrons than protons

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5
Q

What is a cation?

A

An ion with less electrons than protons

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6
Q

Why do ions form?

A

To obtain a full outer shell of electrons

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7
Q

What is the stability of an atom with a full outer shell?

A

More energetically stable

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8
Q

How is electron structure related to an element’s group and period?

A

It determines the element’s chemical properties

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9
Q

What does the Bohr model illustrate?

A

How electrons fill in shells

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10
Q

What do elements in the same group have in common?

A

Same valence shell configuration

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11
Q

What forms ionic compounds?

A

Metals and non-metals

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12
Q

What occurs during bonding in ionic compounds?

A

Transfer of electrons from a metal to a non-metal

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13
Q

What happens to metals in ionic bonding?

A

They lose electrons to form cations

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14
Q

What happens to non-metals in ionic bonding?

A

They gain electrons to form anions

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15
Q

What is true about the overall charge of an ionic compound?

A

It is neutral

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16
Q

How is the number of anions and cations in a compound determined?

A

By the need to cancel positive and negative charges

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17
Q

What holds anions and cations together?

A

Electrostatic force

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18
Q

How is an anionic compound named?

A

Metal first, followed by non-metal with suffix -ide

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19
Q

How do you write the formula for compounds with polyatomic ions?

A

Based on the number of each ion required

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20
Q

What is unique about transition metals regarding cation formation?

A

They can form cations of more than one charge

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21
Q

What do Roman numerals denote in the naming of transition metals?

A

Charge on the transition metal

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22
Q

How can you determine a transition metal’s charge in a compound?

A

By finding how much positive charge cancels the anion’s negative charge

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23
Q

What forms covalent compounds?

A

Non-metals

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24
Q

How does the valence electron shell fill in covalent bonding?

A

By sharing electrons between atoms

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25
What constitutes a covalent bond?
A pair of shared valence electrons
26
How does a non-metal's anionic charge affect bonding?
Determines how many bonds it must form
27
What does a Lewis diagram show?
All valence shell electrons in an atom
28
What does a Lewis bonding diagram represent?
Electrons shared between atoms and non-bonding electrons
29
What does a bonding diagram indicate?
Amount of bonds between each atom using a solid line
30
How are covalent compounds named?
Based on periodic table position with the second element's suffix changed to -ide
31
What prefixes are used when naming covalent compounds?
* mono * di * tri * tetra * penta * hexa
32
Draw the Bohr model for a Beryllium atom (Be)
33
Draw the Bohr model for a Potassium ion (K+)
34
Draw the Bohr model for a Chloride ion (Cl-)
35
What should be drawn for each element: Lithium, Nitrogen, Magnesium, Boron, Fluorine, Sodium, Potassium?
Electron configuration and predict if it will form an anion or cation
36
Explain the relationship between group number and number of valence electrons.
37
Explain the relationship between period number and number of electron shells.
38
Explain the relationship between position in the periodic table and metallic/non-metallic properties.
39
Write the formula for the compound formed between Calcium and fluorine.
40
Write the formula for the compound formed between Sodium and sulfur.
41
Write the formula for the compound formed between Aluminium and oxygen.
42
Write the formula for the compound formed between Potassium and nitrogen.
43
Write the formula for the compound formed between Magnesium and chlorine.
44
Write the formula for the compound formed between Iron(III) and oxygen.
45
Draw electron dot diagrams for NH3 and Phosphorus trichloride.
46
Draw electron dot diagrams for Carbon disulfide and H2.
47
Draw electron dot diagrams for CCl4 and SO2.
48
Identify the bonding type for Potassium oxide.
49
Identify the bonding type for Chlorine gas.
50
Identify the bonding type for AgNO3.
51
Identify the bonding type for NaCl.
52
Explain the difference between the bonding in NaCl and H2O.
53
Complete the table with nuclide symbols for Iodine, Sodium, Selenium, Aluminium, C, Lithium, Argon.
54
Draw the Bohr model for a Sodium atom.
55
Draw the Bohr model for a Potassium ion.
56
Draw the Bohr model for a Nitrogen atom.
57
Draw the Bohr model for an Oxygen ion.
58
Draw the Bohr model for a Calcium ion.
59
Draw the Bohr model for a Sulfur ion.
60
Compare group I and II metals (reactivity, appearance, structure, etc.).
61
What is meant by a 'low energy state' when atoms form ions?
62
Describe the attractive force observed in ionic bonding.
63
Write the name or chemical formula for Sodium sulfate.
64
Write the name or chemical formula for Ca(OH)2.
65
Write the name or chemical formula for Aluminium sulfide.
66
Write the name or chemical formula for Al2(SO4)3.
67
Write the name or chemical formula for Iron (II) chloride.
68
Write the name or chemical formula for CuSO4.
69
Write the name or chemical formula for Manganese (II) hydroxide.
70
Write the name or chemical formula for VO2.
71
Write the name or chemical formula for Chromium (I) oxide.
72
Write the name or chemical formula for Mercury (II) phosphate.
73
Describe the type of bonding within a carbonate anion.
74
Describe the type of bonding between the carbonate anion and sodium cation.

chemistry (2 decks)

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