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Science > Bonding Stucture And Properties Of Atoms > Flashcards

Bonding Stucture And Properties Of Atoms Flashcards

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1
Q

Are ions a charged particle?

A

Yes

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2
Q

How many electrons does group 1 have to 7 have?

A
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3
Q

What is the equation to gain or loss of electron?

A

Losing:
Na -> na+ + e-

Gain
Cl + e- —> Cl-

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4
Q

why are ions attracted to other ions with opposite charge?

A

Due to electrostatic forces

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5
Q

What is the formula for hydroxide ion?

A

OH-

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6
Q

What is the formula for sulfate ion ?

A

SO4[2-]

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7
Q

What is the formula for nitrate?

A

NO3-

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8
Q

What is the formula for carbonate

A

CO3[2+]

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9
Q

What is the formula for ammonium?

A

NH[4+]

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10
Q

What are covalent bonds ?!!!

A

Non metallic atoms which share electrons to gain a full outer shell. These bonds are strong, although have weak intermolecular forces. So they can easily separate.

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11
Q

Name covalent bonds(3)?

A

Water, ammonia, methane

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12
Q

What are the properties of giant covalent structures?

A

-has high melting and boiling point
-cannot conduct electricity
-strong covalent bonds
-has no weak intermolecular forces
-arranged in lattice structure

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13
Q

What are the properties of weak intermolecular structures?

A

-Low boiling and melting point
-has weak intermolecular structures
-cannot conduct electricity
-strong covalent bonds between atoms

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14
Q

What are allotropes?

A

different structural forms of the Same element in the same physical state

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15
Q

What are the properties of a diamond?

A

•each carbon atom covalently bonded to4 other carbon atoms
•strong
•high melting point
•not any free electrons
•does not conduct electricity

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16
Q

What are the properties of graphite?

A

•bonded to 3 carbon atoms
• form flat sheet that is layers with weak intermolecular forces
•soft
•high melting point
•strong individual layers
•has delocalised electrons
•can conduct electricity

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17
Q

What is graphine?

A

A layer of graphite

18
Q

What are the properties of graphene?

A

-Has 3 strong covalent bonds per atom
-strong
-conduct’s electricity

19
Q

What are fullerenes?

A

Made from graphene to form spheres and tubes?

20
Q

What are the properties of fullerene?

A

-Large surface area: volume ratio
-long diameter. Which adds strength with weight

21
Q

What can fullerene be used for?

A

•Industrial catalysts
•Nanotechnology
•materials(tennis racket)
• to transport drugs into body

22
Q

What was the first fullerene called

A

Buckminster fullerene c[60]

23
Q

What are some examples of allotropes?

A

-graphite
-fullerene
-diamond
-graphene

24
Q

What is metallic bonding?

A

When metals bond to other metals.
Each atom becomes an ion with a positive charge, delocalising the electron on the outer shell.

25
Q

What are the properties of metallic bonds?

A

-strong
-high melting point
-can conduct electricity
-can conduct heat
-is malleable(reform shape)

26
Q

What are alloys?

A

Two or more different metals mixed together. As the metals are different sizes, This disrupts regular structure, meaning Layers can’t slide. So they have higher strength than pure metal

27
Q

What is the particle (kinetic) theory?

A

It considers each particle as small, solid and inelastic spheres

28
Q

What are solids?

A

They have regular lattice shape with strong forces of attraction. Which holds particles in a fixed position. Making there shape and volume definite

This means particles can only vibrate in position. However if they vibrate too much, then they will gain more energy and reach a melting point, which begins to break the bonds into a liquid

29
Q

What are liquids?

A

They have weak forces of attraction, which are compact and free to move. There shape can change to fill container.

Although when gaining more heat, particles move faster . That weaken bonds, making them reach a boiling point which breaks bonds into a gas

or when freezing, there is a lack of energy to overcome the forces, which fix the particles in a definite place

30
Q

What are gases?

A

Gases are particles which ‘constantly move with random motion’. They have weak forces of attraction and don’t have a definite shape. Always will fill a container

when heated up will either expand or increase the pressure of the particles

when cooled down, there will not be enough energy to overcome forces, which create bonds between the particles, liquid

31
Q

What has the same electronic structure as sulfur?

A

Argon

32
Q

What force holds ionic bonds together?

A

Electrostatic forces

33
Q

How can you tell particles in a dot and cross diagram are held together by ionic bonds?

A

The particles in compounds are oppositely charged ions

34
Q

What type of structure do ionic compounds have?

A

Giant ionic lattice structure

35
Q

How do ionic bonds form between a non metal and metal?

A

Metal atoms transfer electrons to non metal

-metal becomes positive ion
-non metal becomes negative ion

-the oppositely charged ions are attracted to each other by electrostatic forces of attraction

36
Q

What are the uses for a cross and dot diagram?

A

-shows charge of ions
-shows correct empirical formula
-shows arrangement of electrons in atoms
-shows which atoms the electrons in ion originally come from

37
Q

What are limitations if dot and cross diagram

A

Doesn’t show actual size of ion nor the correct structure

38
Q

What is sort of a ionic compound structure?

A

-has positively charged metals ions and negatively charged non metals ion, in giant ionic structure.

The oppositely charged ions are held together by electrostatic forces that act in all directions

39
Q

What are DSV and ADV of ionic lattice structure?

A

-shows 3D arrangements of ions but doesn’t accurately portray size of ions

40
Q

Why do ionic structures do not conduct electricity when soldi but do when liquid?

A

-Solid: ions in fixed position in lattice structure. So can’t move around and carry charge in solid

-liquid: particles are more free to move so can carry charge to different places

Science (24 decks)

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