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Grade 11 > Chemistry > Flashcards

Chemistry Flashcards

1
Q

what is sedimentation?

A

the process in which solids settle to the bottom of a container.

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2
Q

What is sieving?

A

Separating solid particles according to particle size by passing through a perforated barrier.

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3
Q

What is distillation?

A

The process of separating the liquid component of a solution by boiling the solution and condensing the resulting vapor back to a liquid.

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4
Q

What is decantation?

A

the process of carefully pouring off the liquid and leaving the solid undisturbed at the bottom of the container.

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5
Q

What is filtration?

A

The process of separating undissolved solid from a liquid by passing the mixture through a filter.

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6
Q

What is magnetic separation?

A

The process of passing a mixture through a magnetic field to separate the magnetic and non-magnetic components.

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7
Q

What is evaporation?

A

The process of separating dissolved solid from a solution by vaporising the liquid.

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8
Q

What is crystallisation?

A

The process of forming crystals from a solution.

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9
Q

What properties do we use when separating particles of different size?

A

sieving

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10
Q

What properties do we use when separating solids from liquids?

A

Filtration, decantation.

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11
Q

What properties do we use when separating dissolved solids from liquid?

A

Evaporation or crystallisation

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12
Q

What physical properties do we use when separating two or more liquids?

A

Distillation

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13
Q

What physical properties do we use when separating immiscible (don’t dissolve in one another) liquids?

A

Separating funnel.

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14
Q

Work done by John Dalton?

A
  • 1804, proposed that tiny particles called atoms were the fundamental particles of nature.
  • His theory was that atoms of elements were solid and indivisible.
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15
Q

Who did work to discover established that atoms consist of protons neutrons and electrons?

A

Thompson (plum pudding model), Rutherford and Bohr.

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16
Q

About the nucleus of an atom:

A
  • Positively charged
  • Contains protons and neutrons.
  • Electrons are negatively charged.
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17
Q

How are atoms electrically charged?

A

Neutral.

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18
Q

Proton- mass, relative mass and relative charge

A

1.673 x 10^-27
1
+1

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19
Q

Neutron- mass, relative mass, relative charge.

A

1.673x10^-27
1
0

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20
Q

Electron- mass, relative mass and relative charge

A

9.11x10^-31
0
1

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21
Q

What does the atomic number illustrate about the atom?

A

The number of protons in the nucleus.

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22
Q

What is the mass number?

A

The total number of protons and neutrons.

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23
Q

What are isotopes?

A

Isotopes are different forms of an element. All the atoms of a given element have the same number of protons but the number of neutrons may vary. Different forms of an element may have a different mass number.

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24
Q

What is an element?

A

Elements are substances that contain only one type of atom.

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25
Q

What are compounds?

A

Compounds contain two or more elements, joined together by chemical bonds.

26
Q

What differs compounds from elements?

A

Compounds have properties which are different from the element they contain.

27
Q

What is the periodic law?

A

The properties of the elements are a periodic function of their relative atomic masses.

28
Q

How is the modern periodic table assembled?

A

The elements are in strict order of their atomic numbers. It is divided into vertical groups of similar elements and five blocks of elements with similar properties.

29
Q

What causes elements to have similar properties?

A

Electrons, the valence electrons.

30
Q

What is the letter order of the orbitals?

A

1s, 2s 2p, 3s 3p 3d, 4s

31
Q

What is the exception to the letters of the orbitals?

A

The 4s shell must be filled before filling the 3d shell.

32
Q

How many electrons can each letter orbital have?

A

s-2
p-6
d-10

33
Q

How do elements become noble gases?

A

Metals tend to LOSE electrons to attain a noble gas configuration, whereas non-metals tend to GAIN ELECTRONS. The noble gases neither lose nor gain electrons because THEY ARE STABLE WITH A FILLED SHELL.

34
Q

What two elements are an exception to the orbital rule, with their 3d shell being filled or half-filled before their 4s?

A

Chromium and Copper

35
Q

What is a bond?

A

The electrostatic force that holds atoms, ions or molecules together.

36
Q

How is the type of bond between atoms determined?

A

The type of bond that exists between atoms depends on the electron configuration.

37
Q

How are bonds formed?

A

Formed by the behavior of VALENCE ELECTRONS

38
Q

What are the three sorts of bonds?

A
  • Ionic
  • Covalent-molecular or network
  • Metallic
39
Q

What is ionic bonding?

A

Bonding between metals and non-metals.

40
Q

What is electronegativity?

A

A measure if how well an atom can attract electrons

41
Q

Why can metals and non-metals ionically bond?

A

Because metal atoms have a low number of valence electrons and a low electronegativity. Non-metal atoms have numerous valence electrons.

42
Q

How do metals behave during ionic bonding?

A
  • Lose valence electrons
  • Achieve a stable valence shell (usually 8e-)
  • Gains a positive charge, cation or positive ion.
43
Q

How do non-metals behave during ionic bonding?

A
  • Gain valence electrons
  • Achieve a stable valence shell
  • Gains a negative charge - anion or negative ion.
44
Q

What is the ionic lattice?

A
  • Positive and negative ions attract each other to form a three dimensional continuous lattice structure.
  • The ratio of cations to anions in the lattice is determined by the charges of the ions.
45
Q

Name the seven radicals:

A 
NO3- Nitrate
OH- Hydroxide
SO4 2- Sulfate
CO3 2- Carbonate
PO4 3- Phosphorus
HCO3- Hydrogen Carbonate
NH4+ Ammonium
46
Q 
State the following properties of ionic compounds:
Melting and boiling points:
Electrical Conductivity:
Hardness:
Brittleness:
A
  • High because large amount of thermal energy required to separate ions which are bound by strong electrostatic forces.
  • Solids do not conduct electricity, no mobile charged particles. When molten and in solution, ions are able to carry electric charge and conduct electricity.
  • Most are hard, not easily scratched, aren’t easily displaced
  • Most are brittle, will shatter
47
Q

What is Covalent Molecular bonding?

A

Bonding between two non-metals. All atoms have fairly high electronegativity and few vacancies in valence energy levels. Electrons shared to achieve stable configuration.

48
Q

State the following properties of covalent molecular compounds:
Melting and boiling points:
Electrical Conductivity:
Hardness:

A
  • Low because molecules become separated with little thermal energy.
  • Do not conduct-no mobile charges particles.
  • Soft, weakly attracted and easily displaces
49
Q

What are the prefixes attached to covalent molecular bonds?

A 
1 mono
2 di
3 tri
4 tetra
5 penta
6 hexa
7 septa
50
Q

How are atoms shared in covalent molecular bonds?

A

Electron pairs are shared equally between atoms of equal electronegativity.

51
Q

What is a coordinate covalent bond?

A

Where two electrons are shared evenly with the other atom.

52
Q

What happens if atoms in a covalent bond have differing electronegativities?

A

Electron pairs are attracted closer to the atom with the higher electonegativity value.

53
Q

What happens to the atoms losing and gaining electrons?

A

Atom gaining electrons acquires a slight negative charge (delta -ve)
Atom losing electrons acquires a slight positive charge (delta +ve)
The bond is polar

54
Q

What is covalent network bonding?

A

Bonding between non-metals, form covalent bonds. Do not form separate molecules but a continuous network

55
Q

State the following properties of covalent network compounds:
Melting and boiling points:
Electrical Conductivity:
Hardness:

A
  • Very high melting point, each atom bound by strong covalent bond
  • Poor conductor, electrons cannot move through the lattice (except graphite) approx. 3000
  • Hard
56
Q

What is a metallic bond?

A
  • Transition metals
  • The interaction that holds metal atoms in one piece.
  • Characterised by low ionistion energy
57
Q

What is ionisation energy?

A

The energy required to remove the most loosely held electron from an atom in the gaseous phase.

58
Q

State the properties of metallic compounds:

A
  • dense (heavy)
  • high melting and boiling points
  • Good conductors of heat and electricity
  • Malleable and ductile (bendy)
  • Lustrous (shiny)
59
Q

What is the test for carbon dioxide?

A

turn lime water milky

60
Q

What is the test for hydrogen?

A

Squeaky pop

61
Q

What is melting point related to?

A

The electrostatic attraction in the bonds.

Grade 11 (6 decks)

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