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chem unit 1 > ch 4- reactions of ionic compounds > Flashcards

ch 4- reactions of ionic compounds Flashcards

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1
Q

How does Ionic bonding work

A

-In ionic bonding=Metal atoms donate their valence electrons to non-metal atoms to form cations and anions.
-Cations are electrostatically attracted to anions.
-Ionic compounds(salts have no overall charge.)

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2
Q

Ion(n.)

A

An atom that has lost or gained electrons to become a charged particle

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3
Q

Cation(n.)

A

A positively charged ion formed when one or more valence electrons are lost.

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4
Q

Anion(n.)

A

A negatively charged ion formed when an atom gains one or more valence electrons.

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5
Q

What is an Ionic crystal lattice

A

:A three-dimensional crystal lattice formed when cations and anions combine as solids.

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6
Q

What structure is formed when cations and anions combine as solids

A

An Ionic crystal lattice

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7
Q

Ionic crystal lattice(n.)

A

-Ionic crystal lattice(n.)=symmetrical three-dimensional arrangement of ions.

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8
Q

Coordination number(n.)

A

-Coordination number(n.)=The number of atoms molecules or ions bonded to a chemical species.

E.g.
:Each sodium ion is surrounded by 6 chloride ions and vice versa.
:For sodium chloride, the coordination number is 6.

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9
Q

What are the four properties of ionic compounds

A

There are four properties of Ionic compounds:
1)Brittle
2)Hardness
3)High melting point
4)No electrical conductivity as a solid

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10
Q

Brittle(n.)

A

-Brittle(n.)=The tendency of a material to fracture (break) when subjected to pressure

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11
Q

Hardness(n.)

A

-Hardness(n.)=Resistance to deformation when subject to pressure

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12
Q

High melting point(n.)

A

-High melting point(n.)=The temperature at which a substance changes its state from solid to liquid

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13
Q

Electrical conductivity(n.)

A

-electrical conductivity(n.)=A measurement of how easily a material allows an electrical current to flow through it.

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14
Q

Examples of ionic compounds

A

Sodium chloride = NaCl
Aluminium oxide = Al2O3
Magnesium oxide =MgO

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15
Q

As solids, can ionic compounds conduct electricity?

A

Ions are unable to move, therefore electricity cannot flow through the substance.

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16
Q

As liquids, can ionic compounds conduct electricity?

A

A current can flow through a molten ionic compound

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17
Q

If ionic compounds are dissolved in water, can ionic compounds conduct electricity?

A

A current can flow through an ionic compound in a solution

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18
Q

If ionic compounds are dissolved in any substance, can they conduct electricity?

A

A current can flow through an ionic compound in a solution

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19
Q

What is electricity

A

Electricity is the flow of charge. This can be the flow of electrons, or in the case of ionic substances, the flow of ions.

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20
Q

-Elemental ion(n.)

A

-Elemental ion(n.)=Atom that has lost or gained electrons to become a charged particle

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21
Q

-Species(n.)

A

-Species(n.)=a type of atom, molecule or ion

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22
Q

-Anion(n.)

A

-Anion(n.)=Negatively charged ion formed when an atom gains one or more valence electrons.

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23
Q

-Cation(n.)

A

-Cation(n.)=Positively charged ion formed when one ore more electrons are lost.

24
Q

Electrovalency(n.)

A

-Electrovalency(n.)=Valency of an ion after electron transfer.

25
Q

What does an element having variable electrovalencies mean

A

That the element can form multiple ions with different charges.

26
Q

What are elements that have variable electrovalencies

A

Transition metals(group 3-12) have variable electrovalencies except for Zn^+2, Ag^+

27
Q

What is used to signify the charge of a transitional metal

A

Roman numerals are used with the name to signify the charge on the ion.

E.g. Iron(II)

28
Q

How do you name an ionic compound

A

Cations name stays the same, followed by the anion of the elements ending in ide.

For example
Iron(II) + Oxygen -> Iron(II) Oxide

29
Q

What are polyatomic ions

A

-Polyatomic ion(n.)=Two or more non-metal atoms covalently bonded with an overall charge.

30
Q

Ammonium ion chemical formula

A

NH4 ^+

31
Q

Hydroxide ion chemical formula

A

OH ^-

32
Q

Nitrate ion chemical formula

A

NO3 ^-

33
Q

Hydrogen carbonate ion chemical formula

A

HCO3 ^-

34
Q

Carbonate ion chemical formula

A

CO3 ^2-

35
Q

Sulfate ion chemical formula

A

SO4 ^2-

36
Q

Phosphate ion chemical formula

A

PO4 ^3-

37
Q

When balancing ionic compound equations what must occur

A

The ionic compound created must have no overall charge

38
Q

When naming iodic compounds what is the order, anion and then cation, or then cation then anion.

A

name cation first, followed by the anion

39
Q

Precipitate(n.)

A

-Precipitate(n.)=Precipitate is an insoluble product that is made when substances in solutions are mixed

40
Q

Can two ionic solutions swap their partners to form new ionic compounds

A

:Sometimes two ionic solutions will swap partners to form new ionic compounds
:If an insoluble product is made, this is called precipitate

41
Q

Precipitate(n.)

A

-Precipitate(n.)=A solid that forms when two ionic solutions are mixed

42
Q

Qualitative(n.)

A

-Qualitative(n.)=A factor or variable that is non-numeric e.g. colour

43
Q

Sometimes two ionic solutions will swap partners to form new ionic compounds, what are the characteristics of these two ionic solutions products.

A

-Both of these ionic solutions could produce to other ionic solutions

-One of the ionic compounds can form a precipitate, which is a solid. The other ionic compound remains in solution

44
Q

Full balanced equations(n.)

A

-Full balanced equation(n.)=Balanced equation showing all reactants and products in a reaction including non-reacting species

45
Q

Steps for writing a full equation for precipitate reactions

A

1:Write the formula for the two ionic solutions
2:Swap partners to predict what the products would be in a precipitation reaction
3:Balance the equation

46
Q

Solubility table(n.)

A

-Solubility table(n.)=A table showing which ionic compounds are likely to be soluble or insoluble in water at 25°C

47
Q

States(n.)

A

-States(n.)=Physical form of species, solid(s), Liquid(l), gas(g) or aqueous(aq).

48
Q

How can you identify if a precipitate will form

A

The solubility of the products of two ionic solutions can identify if a precipitate forms

49
Q

What state are precipitates and aqueous ionic compounds denotated as in chemical equations

A

:The precipitate is assigned a (s) state.
:The other ionic compound remains aqueous (aq)

50
Q

Solubility tables mnemonics

A

PANES=ions highly soluble in water
P=Potassium (K)^+
A=Ammonium (NH4)^+
N=Nitrate (NO3)^-
E=Ethanoate (CH3COO)^-
S=Sodium (Na)^+

CHOPS=ions not soluble in water
C=Carbonate (CO3)^2-
H=Hydroxide (OH)^-
O=Oxide (O)^2-
P=Phosphate (PO4)^3-
S=Sulfide (S)^2-

51
Q

Spectator ions(n.)=

A

Spectator ions(n.)=Ions that do not participate and do not change state in a chemical reaction

52
Q

Ionic equation(n.)=

A

Ionic equation(n.)=Equation showing only the species that react. Contains one ore more ions.

53
Q

Steps for writing an ionic equation

A

1.Write the formula for the two ionic substances
2.Swap the partners to predict what the products would be in a precipitation reaction
3.Identify the spectator ions
4.Exclude the spectator ions
5.Summarise the equation as balanced ionic equation including states.

54
Q

Ionic equation of AgNO3(aq) + NaCl(aq)

A

Full balanced equation= AgNO3(aq) + NaCl(aq) -> AgCl(s) + NaNO3(aq)
Ionic equation=Ag^+ + Cl^- -> AgCl(s)

55
Q

SNAPE- ALWAYS SOLUBLE

A

Sodium, Nitrate, Ammonia, Potassium, Ethanoate

chem unit 1 (10 decks)

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