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Chemistry Paper 1 > Ionic Bonding > Flashcards

Ionic Bonding Flashcards

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1
Q

What happens to electrons during the formation of an ionic compound between metals and nonmetals?

A

Electrons in the outer shell of the metal atom are transferred

This transfer leads to the formation of cations and anions.

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2
Q

What do metal atoms become when they lose electrons?

A

Positively charged ions (cations)

Cations are formed when metal atoms lose one or more electrons.

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3
Q

What do nonmetal atoms become when they gain electrons?

A

Negatively charged ions (anions)

Anions are formed when nonmetal atoms gain one or more electrons.

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4
Q

How can the electron transfer during the formation of an ionic compound be represented?

A

By a dot and cross diagram

This visual representation shows the transfer of electrons, such as in NaCl.

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5
Q

What is an ion?

A

An atom or group of atoms with a positive or negative charge

Ions are formed by the loss or gain of electrons.

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6
Q

How is a positive metal ion formed?

A

By a metal losing an electron

This process results in the metal becoming positively charged.

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7
Q

How is a negative ion formed?

A

By a non-metal gaining an electron

This process results in the non-metal becoming negatively charged.

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8
Q

What is the atomic number?

A

Proton number, which is the number of protons in an atom

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9
Q

What is the mass number?

A

Nucleon number, which is the number of protons plus neutrons

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10
Q

In a neutral atom, how do the number of protons and electrons compare?

A

Number of protons equals the number of electrons

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11
Q

Fill in the blank: The mass number is equal to the number of protons plus _______.

A

neutrons

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12
Q

True or False: In an ion, a negative charge indicates electrons were lost.

A

False

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13
Q

True or False: The atomic number can also be referred to as the nucleon number.

A

False

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14
Q

How do you determine the number of electrons in an ion?

A
  1. Find the number of protons (same as the proton number)
  2. Determine how many electrons have been lost or gained based on the charge
  3. Calculate the total number of electrons by adding or subtracting from the number of protons
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15
Q

What does a -ve charge indicate about electrons?

A

Electrons have been gained

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16
Q

What does a +ve charge indicate about electrons?

A

Electrons have been lost

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17
Q

In calculating the number of electrons in an ion, what is the first step?

A

Work out how many electrons an atom of the element would have (same as proton number)

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18
Q

Fill in the blank: To find the total number of electrons in an ion, you calculate the number of electrons in the atom plus electrons _______ or minus electrons lost.

A

gained

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19
Q

True or False: The number of electrons in an ion is always equal to the number of protons.

A

False

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20
Q

What is the electronic structure of ions produced by metals in Groups 1 and 2 and nonmetals in Groups 6 and 7?

A

They have the electronic structure of a noble gas (Group 0)

This configuration is stable and is the driving force behind ion formation.

21
Q

What type of ions do Group 1 metals form?

A

Group 1 metals lose 1 electron and form +1 ions

Examples include sodium (Na⁺) and potassium (K⁺).

22
Q

What type of ions do Group 2 metals form?

A

Group 2 metals lose 2 electrons and form +2 ions

Examples include magnesium (Mg²⁺) and calcium (Ca²⁺).

23
Q

What type of ions do Group 6 nonmetals form?

A

Group 6 nonmetals gain 2 electrons and form 2- ions

Examples include oxygen (O²⁻) and sulfur (S²⁻).

24
Q

What type of ions do Group 7 nonmetals form?

A

Group 7 nonmetals gain 1 electron and form 1- ions

Examples include fluorine (F⁻) and chlorine (Cl⁻).

25
Q

What must be true about the overall charge of a compound formed from these ions?

A

A compound will have an overall charge of 0

This requires balancing the positive and negative charges.

26
Q

Fill in the blank: Group 1 metals will lose ______ electron(s) and form +1 ions.

A

1

27
Q

Fill in the blank: Group 2 metals will lose ______ electron(s) and form +2 ions.

A

2

28
Q

Fill in the blank: Group 6 nonmetals will gain ______ electron(s) and form 2- ions.

A

2

29
Q

Fill in the blank: Group 7 nonmetals will gain ______ electron(s) and form 1- ions.

A

1

30
Q

What does the ending -ide signify in the names of compounds?

A

-ide means the compound contains 2 elements, one of which is the nonmetal negatively charged ion.

This naming convention is used in ionic compounds where there is a binary combination of elements.

31
Q

What does the ending -ate signify in the names of compounds?

A

-ate means the compound contains at least 3 elements, one of which is oxygen.

This is commonly used in polyatomic ions, where the compound includes a central atom bonded to multiple oxygen atoms.

32
Q

What type of ions do the endings -ide and -ate refer to in compounds?

A

They refer to negatively charged ions in a compound.

These endings help categorize the type of ion present in the compound.

33
Q

What is the ion involved in the formation of an oxide?

A

O’ ion

Example: sodium oxide is Na2O

34
Q

What ion is present in hydroxides?

A

OH’- ion

Example: sodium hydroxide is NaOH

35
Q

What type of ion is a halide?

A

-1 halide ion

Example: sodium chloride is NaCl

36
Q

What ion is involved in the formation of nitrates?

A

NO3’ ion

Example: sodium nitrate is NaNO3

37
Q

What ion is present in carbonates?

A

CO3’ ion

Example: sodium carbonate is Na2CO3

38
Q

What ion is involved in the formation of sulfates?

A

SO4’ ion

Example: sodium sulfate is Na2SO4

39
Q

What is required to deduce the formula of ionic compounds?

A

Balance the + and - charges to make the overall charge 0

This involves adjusting the subscripts of the ions

40
Q

How do you denote ions with more than one element when writing formulas?

A

Draw a bracket around the ion

For example: (SO4)2

41
Q

What is the structure of an ionic compound?

A

A lattice structure consisting of a regular arrangement of ions held together by strong electrostatic forces (ionic bonds) between oppositely charged ions.

42
Q

What type of structure do ionic compounds form?

A

A giant structure of ions.

43
Q

What type of forces hold ionic compounds together?

A

Strong electrostatic forces of attraction.

44
Q

What is ionic bonding?

A

The forces that act in all directions in the lattice between oppositely charged ions.

45
Q

What is a characteristic feature of the ionic lattice arrangement?

A

A regular arrangement of ions.

46
Q

Fill in the blank: An example of an ionic compound is _______.

A

sodium chloride (NaCl).

47
Q

In the example of sodium chloride, what are the charges of the ions involved?

A

Na+ (positive) and Cl- (negative).

48
Q

True or False: The ions in an ionic compound are randomly arranged.

A

False.

49
Q

What type of particles are Na+ and Cl- in sodium chloride?

A

Na+ are small blue particles and Cl- are larger green particles.

Chemistry Paper 1 (7 decks)

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