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Chemistry > C2 > Flashcards

C2 Flashcards

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1
Q

What is relative atomic mass?

A

Relative atomic mass, Ar, is the mean mass of an element compared to 1/12 the mass of a carbon-12 atom

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2
Q

What is relative formula mass?

A

Relative formula mass, Mr, is the mean mass of a unit of substance compared to 1/12 the mass of a carbon-12 atom

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3
Q

What is relative molecular mass?

A

Relative molecular mass, Mr, is the mean mass of a unit of a molecule compared to 1/12 the mass of a carbon-12 atom

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4
Q

Appearance of metals and non-metals

A

Metals are shiny, non-metals are dull

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5
Q

Melting and boiling point of metals and non-metals

A

Metals usually have high melting and boiling points, while non-metals are usually low

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6
Q

State at room temperature for metals and non-metals

A

Metals are solid, non-metals have half solid, half gas

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7
Q

Malleable or brittle when solid for metals and non-metals

A

Metals are malleable, non-metals are brittle

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8
Q

Ductile or non-ductile when solid for metals and non-metals

A

Metals are ductile, while non-metals are non-ductile

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9
Q

Thermal and electrical conductivity for metals and non-metals

A

Metals are good conductors, non-metals are poor conductors

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10
Q

How do metals and non-metals form ions?

A

Metals lose electrons to form positive ions, while non-metals gain electrons to form negative ions

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11
Q

How do metals and non-metals react with each other?

A

Metals don’t react with each other (mix to form alloys) while non-metals react to produce compounds that consist of molecules

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12
Q

What types of solutions do metals and non-metal oxides form when placed in water?

A

Metal oxides form alkaline solutions

Non-metal oxides produce acidic solutions

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13
Q

How do ionic compounds form?

A

When a metal reacts with a non-metal, electrons are transferred from the metal atoms to the non-metal atoms so both achieve more stable electronic structures

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14
Q

How are ionic compounds structured?

A

Ionic compounds contain positive and negative ions arranged in a regular way. This is called a giant ionic lattice

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15
Q

How are ions in ionic compounds held in place?

A

Ions are held in place by ionic bonds, which are electrostatic forces of attraction between oppositely charged ions

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16
Q

What are the limitations of dot and cross diagrams?

A

Dot and cross diagrams don’t show the 3D structure

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17
Q

What are the limitations of ball and stick models?

A

Ions are close together, and bonds are forces rather than physical objects made from matter, size is exaggerated

18
Q

What are covalent bonds and how do they form?

A

Covalent bonds are shared pairs of electrons, which form between two non-metal atoms when the atoms get close enough to share electrons, to complete their outer shells

19
Q

What are simple molecules?

A

Simple molecules are molecules that contain only a few atoms

20
Q

What are the forces in covalent bonds?

A

In covalent bonds, they involve electrostatic forces of attraction between the nucleus of each bonded atom and the shared electrons

21
Q

The … between atoms in a simple molecule are …, but the … are …

A

covalent bonds, strong, intermolecular forces, weak

22
Q

What are the limitations of a displayed formula?

A

A displayed formula doesn’t show the shape of the simple molecule, or the 3D part of it

23
Q

What are giant covalent structures?

A

Giant covalent structures consist of many non-metal atoms joined by covalent bonds

24
Q

How are atoms arranged in a giant covalent structure?

A

In a repeating regular pattern called a giant covalent lattice

25
Q

What are the chemical formulae of giant covalent structures?

A

They are represented as empirical formulae because there are so many atoms

26
Q

What are polymers?

A

Polymers are molecules that join end to end from smaller molecules called monomers

27
Q

How are polymer molecules modelled?

A

Polymers are modelled using their monomer form, using dot and cross, space filling and ball & stick models

28
Q

What are repeating units?

A

Repeating units are sections of a polymer that is repeated over and over again, rather like links in a chain

29
Q

What are the structure of metals like?

A

Metal atoms are packed together in a regular way, forming a giant metallic lattice

30
Q

How can you model a metal?

A

By drawing circles or spheres arranged in a regular pattern

31
Q

What are metallic bonds?

A

Metallic bonds are the strong electrostatic forces between delocalised electrons and the closely packed, positively charged metal ions

32
Q

What are the limitations of the isometric diagram of the metal?

A

An isometric diagram doesn’t show the delocalised electrons, and the subatomic particles overlap

33
Q

What are the limitations of the elevation view of the metal?

A

It doesn’t show the 3D structure of the metal of the metallic bonding it has

34
Q

How are the reactions of elements related to the arrangement of electrons in the atoms?

A

As elements lose or gain certain numbers of electrons in order to complete their outer shells in reactions

35
Q

How are reactions of elements related to the atomic number?

A

As the number of electrons before the reaction represents the atomic number

36
Q

Groups 1 and 2 become … reactive as you go down the group

A

more

37
Q

Group 7 becomes … reactive as you go down the group

A

less

38
Q

What was Mendeleev’s first arrangement of the periodic table?

A

Mendeleev’s arranged all the elements known in order of atomic weight, and he grouped the ones with similar chemical properties

39
Q

How was Mendeleev’s arrangement refined?

A

He rotated his table so the groups were shown as columns

40
Q

What did Henry Moseley do and what did this lead to?

A

Henry Moseley discovered that an atoms atomic number was the number of protons in its nucleus, and this led to the creation of the modern Periodic Table

Chemistry (4 decks)

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