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chemistry > The Particulate Nature of Matter > Flashcards

The Particulate Nature of Matter Flashcards

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1
Q

does gas and liquid have a fixed shape?

A

no, only solid have fixed shapes

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2
Q

describe the movement of particles in liquids?

A

particles slide past each other

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3
Q

describe the movement of particles in gases?

A

particles move rapidly and randomly

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4
Q

what are the states of matter?

A

solid, liquid and gas

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5
Q

describe the movement of particles in a solid?

A

particles vibrate about a fixed position

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6
Q

describe the arrangement of particles in a liquid?

A
  • closely packed
  • disorderly manner

https://tse4.mm.bing.net/th?id=OIP.AxYNKAX_FJcxiDYXxZk31QHaD2&pid=Api&P=0&h=180

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7
Q

describe the arrangement of particles in a solid

A
  • very closely packed
  • orderly manner

https://tse4.mm.bing.net/th?id=OIP.AxYNKAX_FJcxiDYXxZk31QHaD2&pid=Api&P=0&h=180

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8
Q

describe the arrangement of particles in a gas?

A
  • disorderly
  • very far apart
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9
Q

attractive forces between particles of a solid?

A

very strong

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10
Q

attractive forces between particles of a liquid

A

strong

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11
Q

attractive forces between particles in a gas

A

very weak

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12
Q

Guidelines to draw particles

A
  • At least 75% of space should be covered
  • At least 9 particles drawn (for solid & liquid states)
  • Minimum 3 for gaseous state
  • All particles are to be of the same size
  • Space between any 2 particles should be smaller than the size of 1 particle
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13
Q

What is the relative charge and mass of a proton?

A

relative charge: +1
relative mass: 1

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14
Q

What is the relative charge and mass of a Neutron?

A

relative charge: 0
relative mass: 1

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15
Q

What is the relative charge and mass of a Electron?

A

relative charge: -1
relative mass: 1/1840

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16
Q

What is sublimation?

A

We can define sublimation as the transition of a substance from the solid phase to the gaseous phase without changing into the liquid phase.

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17
Q

define proton (atomic) number

A

The number of protons in the atom

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18
Q

Define mass number/Nucleon Number

A

The total number of protons and neutrons in the atom.

19
Q

What do you notice about the number of protons and electrons

A

The number of protons is equal to the number of electrons

20
Q

What are the electrons in the outermost shell called?

A

Valance electrons

21
Q

define the term isotopes

A

Atoms of the same element with the same number of protons and electrons but different number of neutrons.

22
Q

Describe how a magnesium
atom forms a magnesium ion.

Hint: how to make to stable electronic configuration?

A

Electronic structure of magnesium is 2.8.2.
It will lose 2 electrons Ion to form Mg2+ ion and obtain stable electronic configuration
Ionic Equation Mg  Mg2+ + 2e-

23
Q

What are noble gases?

A

Noble gas: group 0 ,
monoatomic gas ,
stable electronic configuration

24
Q

Do metals gain or lose electrons?

hint: picture the periodic table in ur head, how to make metals stable?

A

metals lose electrons

25
Q

Do non-metals gain or lose electrons?

hint: picture the periodic table in ur head, how to make metals stable?

A

gain electrons

26
Q

What is an ionic bond?

A

It is formed by transfer of electrons from metal to non metal

27
Q

What is covalent bond?

A

Sharing of electrons between non metals

28
Q

How is the bond in sodium chloride formed? (use this structure to do other similar qns)

A

Electronic configuration > Electronic configuration of sodium is 2.8.1
and chlorine is 2.8.7.

Process > Sodium atom will transfer 1 valence electron and the Chlorine atom will gain 1 electron

Ion > Sodium will form +1 charge and chloride ion -1 charge

Reason> To obtain stable electronic configuration

29
Q

MUST KNOW covalent structures!

A
  • water
  • Ammonia
  • Carbon Dioxide
  • Methane

note to self: add in picture from pg 5 chapter 10 bonding

30
Q

When to draw ionic compound?

A

When metal and non-metal transfer electrons

31
Q

when to draw covalent compound?

A

when non-metal and non-metal shares electrons

32
Q

What are the physical properties of ionic compound?

A
  • Ionic bonds are formed by transfer of
    electrons from metals to non metal
  • Metal atoms tend to lose electrons to form positive ions. (cations)
  • Non-metal atoms tend to gain electrons to form negative ions. (anions)
33
Q

properties of Ionic compounds

A
  • High melting and boiling point
    Structure > Giant lattice structure
    Attraction > Strong electrostatic forces of attraction between
    Particles >Opposite charged ions
    Energy > More energy needed to
    break these forces
34
Q

Properties of Covalent compound

A
  • Low melting and boiling point
    Structure >Simple molecular structure
    Attraction >Weak intermolecular forces
    of attraction between
    Particles> molecules
    Energy>Less energy needed to
    break these forces
35
Q

State of ionic compound at room temp.

A

Solids at room temp.

36
Q

State of covalent compound at room temp.

A

usually exist as gases or liquids at
room temperature

37
Q

Solubility of Ionic compounds

A
  • soluble in water
  • insoluble in organic solvent
    eg. Oil, alcohol
38
Q

Solubility of Covalent compounds

A
  • soluble in organic solvent
  • insoluble in water
39
Q

Electrical Conductivity of ionic compounds

A

In molten and aqueous states
Reason:
Mobile ions are present as able to move and carry electric current

40
Q

Electrical Conductivity of covalent compounds

A

Does not conduct electricity in any state
Reason:
No mobile ions to carry electric current

41
Q

Why are ionic compounds unable to conduct electricity in a solid state?

A

Ions are held in fixed positions in a giant ionic lattice structure and unable to move

42
Q

Covalent compounds cannot conduct electricity in any state, but there are Exceptions

A

Hydrogen chloride gas dissolves in water to form hydrochloric acid.
In aqueous state, ions are able to move &
carry electric current
Equation: HCl (aq) >H+(aq) + Cl- (aq)

43
Q

Using structure and bonding, explain why the melting point of sodium chloride
(ionic compound) is higher than chlorine gas (covalent compound)?

hint: use SAPE to answer the qn

A

Sodium chloride has giant lattice structure (S) with strong electrostatic forces of attraction between (A) opposite charged ions (P) More energy needed to break these forces (E). Chlorine has has simple molecular structure (S) weak intermolecular forces of attraction between(A) molecules (P). Less energy needed to break these forces.(E)

chemistry (10 decks)

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