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Lecture 6 > Ionic Bonds > Flashcards

Ionic Bonds Flashcards

1
Q

Ionic Meaning

A

transfer of electrons (one loses to another)

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2
Q

What does ionic bonds, bond?

A

usually metal to nonmetal

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3
Q

Covalent meaning

A

sharing of electrons

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4
Q

What does covalent bonds, bond?

A

nonmetal to nonmetal

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5
Q

Metallic meaning

A

sea of electrons

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6
Q

What does metallic bonds, bond?

A

metal to metal

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7
Q

Monatomic ion

A

an ion formed by a single atom

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8
Q

Polyatomic ion

A

an ion formed from more than 1 atom

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9
Q

Binary Compound

A

a compound composed of 2 elements

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10
Q

Why do elements want to form ionic bonds?

A

to achieve noble gas configuration, full valence shell (octet)

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11
Q

What are ionic bonds?

A

ions held together by oppposite charges,

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12
Q

What holds together ionic bonds?

A

electrostatic charge, cations and anions

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13
Q

formula unit

A

simplest ratio of elements in an ionic compound

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14
Q

What are ionic compounds called?

A

salts

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15
Q

What is the total charge of any ionic compound?

A

zero

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16
Q

What can create a stronger bond?

A

higher charges

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17
Q

How does distance effect an ions bond?

A

shorter distance=stronger bond (smaller radii)

18
Q

What is a crystalline solid?

A

a regular repeating arrangement of ions in the solid

19
Q

What are the properties of a crystalline solid?

A

The ions are strongly bonded together; the structure is rigid,

20
Q

properties of ionic compounds

A

crystalline solid, high melting points

21
Q

What is a coordination number?

A

number of ions of opposite charge surrounding it

22
Q

Can ionic compounds conduct electricity?

A

Ionic compounds are usually solid at room temperature, which means they are insulators. Once they are melted or dissolved, they coulf conduct electricity

23
Q

How does melting or dissolving a solid allow for it to conduct electricity?

A

The ions are free to move around, which allows the electric currents to move as well

24
Q

Why are ionic crystals brittle?

A

The oppositily charged particles will slide past eachother, but since like charges repel, it will break apart the crystal.

25
Q

metals are always

A

cations, positive charge

26
Q

nonmetals are always

A

anions, negative charge

27
Q

What does a chemical formula show?

A

the kinds and numbers of atoms in the smallest representative particle of the substance

28
Q

What is written first in a ionic compound?

A

cations, then anion

29
Q

What is the smallest representative particle called?

A

formula unit

30
Q

What metals can have multiple charges?

A

transition-post transition metals (with exceptions)

31
Q

What are the 2 methods of clarifying if the metal has more than 1 charge

A

Stock System and Classical Method

32
Q

What is the Stock System

A

Putting roman numerals after the name (Ex. Copper (II)

33
Q

What is the classical method

A

Using suffixes, -ous & -ic (Ex. Cupric)

34
Q

What are the transition metals with only 1 charge? (Exceptions)

A

Silver Ag+1
Cadmium Cd+2
Zinc Zn+2

35
Q

What the post-transition metals with multiple charges? (Exceptions)

A

Tin (II) Sn+2
Tin (IV) Sn+4
Lead (II) = Pb+2
Lead(IV) = Pb+4

36
Q

Can the charge of the cation change?

A

Yes, since some transition and post-transition metals have multiple charges

37
Q

Can the charge of the anion change?

A

No, all the nonmetals only have 1 charge

38
Q

What do you add to the end of a monatomic element?

A

-ide
(Ex. Fluoride, Oxide, etc)

39
Q

What are Polyatomic Ions?

A

Group of atoms that stay together and have an overall charge and 1 name

40
Q

What do polyatomic ions usually end with?

A

-ate, -ite

41
Q

What are the exceptions to the polyatomic ion naming suffix?

A

Hydroxide OH-
Cyanide CN-
Ammonium NH+4

42
Q

What are the rules of anming an ionic compound?

A
  1. cation, then anion
  2. name of first element (cation), plus charge if needed
  3. name of 2nd element (anion), ending with -ide

Lecture 6 (6 decks)

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