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GCSE OCR CHEMISTRY > 2.2 > Flashcards

2.2 Flashcards

1
Q

What are the two broad types of elements based on their properties?

A

Answer: Metals and non-metals.

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2
Q

What happens to atoms of elements that do not have a full outer shell of electrons in chemical reactions?

A

Answer: They can try to achieve a full outer shell by gaining or losing electrons, leading to the formation of ions.

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3
Q

What is an ion?

A

Answer: An ion is an atom or molecule that has become charged through the loss or gain of one or more electrons.

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4
Q

Do metals form positive or negative ions when they react? Why?

A

Answer: Metals form positive ions when they react because they lose electrons, resulting in fewer negatively charged electrons but the same number of positively charged proto

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5
Q

Do non-metals form positive or negative ions when they react? Why?

A

Answer: Non-metals form negative ions when they react because they gain electrons, resulting in more negatively charged electrons but the same number of positively charged proton

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6
Q

What are elements that display properties of both metals and non-metals called?

A

Answer: Metalloids or semi-metals.

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7
Q

Describe the trend of metallic character across a period on the periodic table.

A

Answer: Metallic character decreases as you move across a period from left to right.

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8
Q

Describe the trend of metallic character down a group on the periodic table.

A

Answer: Metallic character increases as you move down a group on the periodic table.

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9
Q

Question: What is the typical electron arrangement for metals?

A

Answer: Metals typically have 1-3 outer shell electrons

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10
Q

What is the typical electron arrangement for non-metals?

A

Answer: Non-metals typically have 4-7 outer shell elect

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11
Q

What type of bonding is present in metals?

A

Answer: Metallic bonding occurs in metals due to the loss of outer shell electrons.

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12
Q

Question: What type of bonding is present in non-metals?

A

Answer: Non-metals exhibit covalent bonding, where outer shell electrons are shared.

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13
Q

How do metals and non-metals differ in terms of electrical conductivity?

A

Answer: Metals are good conductors of electricity, while non-metals are poor conductors.

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14
Q

What type of oxides do metals typically form?

A

Answer: Metals usually form basic oxides, with some being amphoteric.

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15
Q

How do metals generally react with acids?

A

Answer: Many metals react with acids.

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16
Q

What type of oxides do non-metals typically form?

A

Answer: Non-metals usually form acidic oxides, with some being neutral.

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17
Q

What are some physical characteristics of metals?

A

Answer: Metals are usually lustrous, solid at room temperature (excluding mercury), malleable, and have high melting and boiling points.

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18
Q

What are some physical characteristics of non-metals?

A

Answer: Non-metals are dull, have different states at room temperature, are flaky and brittle, and have low melting and boiling points

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19
Q

How does the number of electrons in the outer shell of metals compare to non-metals on the periodic table?

A

Answer: Metals on the left of the periodic table have fewer electrons in their outer shells compared to non-metals on the right.

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20
Q

What happens to the outer shell electrons as you descend any group on the periodic table?

A

Answer: The outer shell electrons become further away from the nucleus due to increasing atomic size, weakening the attraction between the outer shell electrons and the nucleus.

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21
Q

How does the reactivity of metallic elements change as you descend a group on the periodic table?

A

Answer: Metallic elements become more reactive as you descend a group because they can more easily lose their outer electron(s).

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22
Q

How does the reactivity of non-metallic elements change as you descend a group on the periodic table?

A

Answer: Non-metallic elements become less reactive as you descend a group because it becomes harder for them to attract extra electrons and gain a full outer shell.

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23
Q

What is the key difference in chemical behavior between metals and non-metals?

A

Answer: The ease of losing electrons for metals and gaining electrons for non-metals influences their chemical behavior.

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24
Q

How is an element’s atomic number related to its position on the periodic table and its reactivity?

A

Answer: Elements in Group 1 have one outer shell electron, Group 2 have two outer shell electrons, and so on. This number of outer electrons influences an element’s reactivity.

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25
Q

How are elements arranged on the periodic table?

A

Answer: Elements are arranged in order of increasing atomic number, with each element having one more proton and one more electron than the element preceding it.

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26
Q

What are the horizontal rows on the periodic table called?

A

Answer: The horizontal rows are called periods, and they indicate the number of electron shells an atom has.

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27
Q

What are the vertical columns on the periodic table called?

A

Answer: The vertical columns are called groups, and they indicate how many outer electrons each atom has.

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28
Q

Question: What are some alternative names for certain groups on the periodic table?

A

Answer: Group 1 is known as the ‘alkali metals’, Group 7 is known as the ‘halogens’, and Group 0 is known as the ‘noble gas

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29
Q

What is the outermost shell of an atom called?

A

Answer: The outermost shell is called the valence shell, and atoms are more stable when this shell is completely filled with electrons

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30
Q

How do atoms react to achieve a full outer shell?

A

Answer: Atoms can gain or lose electrons to complete their outer shell, forming ions (anions for non-metals and cations for metals), or they can share electrons to form covalent bonds.

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31
Q

Question: What holds positively and negatively charged ions together in an ionic bond?

A

Answer: The strong electrostatic forces of attraction between the oppositely charged ions hold them together.

32
Q

What types of elements typically form an ionic bond?

A

Answer: An ionic bond occurs between a metal and a non-metal.

33
Q

Question: What are the advantages of dot and cross diagrams for illustrating ionic compounds?

A

Answer: Dot and cross diagrams are useful for illustrating the transfer of electrons and indicating from which atom the bonding electrons come from.

34
Q

What are the disadvantages of dot and cross diagrams for illustrating ionic compounds?

A

Answer: Dot and cross diagrams fail to illustrate the 3D arrangements of the atoms and electron shells, and they don’t indicate the relative sizes of the atoms.

35
Q

What are the advantages of ball and stick models for illustrating ionic compounds?

A

Answer: Ball and stick models are useful for illustrating the arrangement of atoms/ions in 3D space and visualizing the shape of an ionic compound.

36
Q

What are the disadvantages of ball and stick models for illustrating ionic compounds?

A

Answer: Ball and stick models fail at indicating the movement of electrons, the ions are placed far apart from each other which isn’t accurate, the size of ions isn’t accurate, they don’t show the charges on ions, and ions are shown as being physically bonded when they are held together by electrostatic forces of attraction.

37
Q

Question: How do non-metal atoms achieve a full outer shell of electrons?

A

Answer: Non-metal atoms can share electrons with other non-metal atoms to obtain a full outer shell of electrons.

38
Q
  1. Question: What type of bond forms when atoms share pairs of electrons?
A

Answer: When atoms share pairs of electrons, they form covalent bonds.

39
Q

How strong are covalent bonds between atoms?

A

Answer: Covalent bonds between atoms are very strong

40
Q

What do two or more chemically bonded atoms form?

A

Answer: Two or more chemically bonded atoms form molecules.

41
Q

What are some characteristics of covalently bonded substances?

A

Answer: Covalently bonded substances may consist of small molecules or giant structures, and weak intermolecular forces exist between individual molecules.

42
Q

What are shared electrons in covalent bonds called?

A

Answer: Shared electrons are called bonding electrons and occur in pairs.

43
Q

What are electrons on the outer shell that are not involved in covalent bonds called?

A

Answer: Electrons on the outer

44
Q

What are the advantages of dot and cross diagrams for illustrating simple covalent molecules?

A

Answer: Dot and cross diagrams are useful for illustrating the transfer of electrons and indicating from which atom the bonding electrons come from.

45
Q

What are the disadvantages of dot and cross diagrams for illustrating simple covalent molecules?

A

Answer: Dot and cross diagrams fail to illustrate the 3D arrangements of the atoms and electron shells, and they don’t indicate the relative sizes of the atoms.

46
Q

What are the advantages of ball and stick models for illustrating simple covalent molecules?

A

Answer: Ball and stick models are useful for illustrating the arrangement of atoms in 3D space and visualizing the shape of a molecule.

47
Q

What are the disadvantages of ball and stick models for illustrating simple covalent molecules?

A

Answer: Ball and stick models fail at indicating the movement of electrons, and the atoms are placed far apart from each other, which isn’t accurate.

48
Q

What are the advantages of 2D representations of molecules?

A

Answer: 2D representations adequately indicate what atoms are in a molecule and how they are connected.

49
Q

What are the disadvantages of 2D representations of molecules?

A

Answer: 2D representations fail to illustrate the relative sizes of the atoms and bonds, and they cannot give an idea of the shape of a molecule in 3D space

50
Q

What are the melting and boiling points of giant covalent structures?

A

Answer: Giant covalent structures have high melting and boiling points due to many strong covalent bonds.

51
Q

Why do giant covalent structures require large amounts of heat energy to break down bonds?

A

Answer: Large amounts of heat energy are needed to overcome these forces and break down bonds in giant covalent structures.

52
Q

Can most giant covalent structures conduct electricity? Why or why not?

A

Answer: Most cannot conduct electricity as they do not have free electrons nor charged particles, although there are exceptions such as graphite and graphene.

53
Q

What are some special characteristics of diamond?

A

Answer: Diamond is a transparent crystal, it’s the hardest known naturally occurring substance

54
Q

What are some special characteristics of graphite?

A

Answer: Graphite is a grey-black solid, soft, and slippery

55
Q

What are some special characteristics of silicon dioxide?

A

Answer: Silicon dioxide is a semiconductor, a very good conductor, and exists in transparent sheets or cryst

56
Q

What are some special characteristics of buckminster-fullerene?

A

Answer: Buckminster-fullerene has a low melting and boiling point.

57
Q

What are some special characteristics of graphene?

A

Answer: Graphene is very strong and flexible, around 100 times stronger than steel, and exhibits piezoelectricity, producing electric charge from mechanical stress.

58
Q

What are polymers?

A

Answer: Polymers are very large covalent molecules, sometimes called macromolecules, made by linking together large numbers of smaller molecules called monomers.

59
Q

What is a monomer in relation to polymers?

A

Answer: Each monomer is a repeat unit and is connected to adjacent units via strong covalent bonds.

60
Q

What are some characteristics of polymers?

A

Answer: Polymers have high relative molecular mass, and the intermolecular forces acting between polymer chains are larger than those between simple molecules, making them usually solid at room temperature.

61
Q
  1. Question: What are some common examples of polymers?
A

Answer: Common polymers include polythene (used in plastic bags) and polyvinyl chloride (PVC, used in water pipes).

62
Q

What are synthetic polymers?

A

Answer: Synthetic polymers are manufactured materials, such as resins, plastics, and polystyrene cups.

63
Q

What are natural or biological polymers?

A

Answer: Natural or biological polymers are polymers produced by nature, such as DNA, proteins, silk, and wool.

64
Q

How are polymers represented structurally?

A

Answer: Polymers are represented as very long carbon chains with repeating units, as shown in diagrams depicting a section of polystyrene.

65
Q

What method did scientists use to arrange elements before the discovery of subatomic particles?

A

Answer: Before the discovery of subatomic particles, scientists arranged elements in order of their atomic mass, rather than their atomic number.

66
Q

Question: What patterns emerged when elements were arranged by atomic mass?

A

Answer: Some patterns emerged at regular intervals along the table, giving rise to the term “periodic.”

67
Q

: Why were the early periodic tables incomplete?

A

Answer: The early tables were incomplete because not all elements had been discovered. This led to gaps in the table, and some elements were forced into positions to fill these gaps, disrupting the patterns.

68
Q

Why were some elements placed in the wrong group on early periodic tables?

A

Answer: Some elements were placed in the wrong group because they were sorted strictly by mass, ignoring their chemical properties. This resulted in groups not always sharing similar chemical behavior.

69
Q

Question: How did scientists in different countries contribute to the development of early periodic tables?

A

Answer: Scientists in different countries created their own versions of the periodic table as they grappled with the ordering of elements.

70
Q

What was Mendeleev’s role in the development of the periodic table?

A

Answer: Mendeleev worked to improve the periodic table by refining its organizativos and addressing the inconsistencies and gaps present in earlier versions.

71
Q

Question: How did Mendeleev organize the elements on the Periodic Table?

A

Answer: Mendeleev organized the elements into vertical columns based on their chemical properties and the properties of their compounds.

72
Q

What pattern did Mendeleev observe as he arranged the elements horizontally by increasing atomic mass?

A

Answer: Mendeleev observed that chemically similar elements fell naturally into the same columns as he arranged them horizontally by increasing atomic mass.

73
Q

How did Mendeleev handle elements that did not fit the pattern when arranged by atomic mass?

A

Answer: Mendeleev left gaps in the table for elements that did not fit the pattern, predicting that these gaps would be filled by elements that had not yet been discovered.

74
Q

What was unique about Mendeleev’s approach to leaving gaps in the periodic table?

A

Answer: Mendeleev’s approach was unique because other chemists assumed there were no gaps in the table, while Mendeleev anticipated and left gaps for undiscovered elements.

75
Q

How did Mendeleev predict the properties of undiscovered elements corresponding to the gaps in his periodic table?

A

Answer: Mendeleev used the properties and trends of other elements in the group with the gap to predict the properties of undiscovered elements.

GCSE OCR CHEMISTRY (7 decks)

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