C2. The Periodic Table Flashcards
Define the term period in the context of the Periodic Table
A period is a horizontal row in the Periodic Table that shows the number of electrons
What does the group number indicate in the Periodic Table?
Indicates the number of electrons in the outer shell of an element
What is the relationship between group number and the number of electrons in the outer most shell of an atom
The group number is the same as the number of electrons in the outer most shell of an atom
Define the term group in the context of the Periodic Table
Groups are the vertical columns that show how many outer electrons each atoms has
What did the gaps in Mendeleev’s table represent?
The gaps in Mendeleev’s table represented undiscovered elements
What is the modern basis for arranging elements in the periodic table?
Elements in the modern periodic table are arranged by increasing atomic number
Before the discovery of protons, neutrons and electrons how was the early Periodic Table ordered?
Before the discovery of protons, neutrons and electrons the early Periodic Table was ordered by atomic weight
What confirmed Mendeleev’s theories about his Periodic Table?
Mendeleev’s theories about his Periodic Table were confirmed when these elements were later discovered and found to fit in his pattern
What change to the Periodic Table arrangement took place when subatomic particles were discovered?
The arrangement changed by ordering by atomic number rather than atomic mass
In terms of their physical state at room temperature what is the difference between metals and non-metals?
At room temperature, metals are typically solid and non-metals cam be gases or solids
Mercury and bromine are exceptions as they are liquid at room temperature
What properties are used to classify elements as metals or non-metals?
Conductivity
Melting/boiling point
Reaction with acid
Type of oxide formed
Where are non-metals generally located on the Periodic Table?
On the right-hand side of the Periodic Table
What type of oxide do metals normally form?
Metals normally form basic oxides
Do metals or non-metals generally have low melting and boiling points?
Non-metals generally have low melting and boiling points
State the characteristic properties of metals and non-metals?
Metals typically have high electrical conductivity, are malleable/ductile, reacts with acids and form basic oxides
Non-metals typically have lower electrical conductivity, are brittle, do not react with acids and form acidic oxides
What is Group 0 of the Periodic Table called?
Noble gases
Why are noble gases unreactive?
Noble gases are unreactive as they have full outer shells of electrons
What is Group 1 of the Periodic Table called?
Alkali metals
Name the two products formed when sodium reacts with water.
Sodium hydroxide and hydrogen
Give two properties of Group 1 metals
They are soft
They have relatively low densities
They have relatively low melting points
They are very reactive
Explain why the alkali metals share similar chemical properties
The alkali metals share similar chemical properties because they all have one electron/ the same number of electrons in their outer shell.
Describe the trend in reactivity going down Group 1
Reactivity increases
Apart from fizzing/effervescence, state two other observations that would be made when sodium is added to water
Floating
Moving
Melting/turning into a ball/sphere
Getting smaller/disappearing/dissolving
Leaving a white trail
Give the charge of the ions formed when a Group 1 metals loses an electron
1+
Name Group 7 of the Periodic Table
The Halogens
Give the colour and state of chlorine at room temperature
Pale green gas
Describe what happens to the melting points of the halogens going down the group
The melting point of the halogen increases
What is meant by a halogen displacement reaction?
Where a more reactive halogen displaces a less reactive halogen form an aqueous solution of its halide
Explain why chlorine has a higher melting point than fluorine
Chlorine has a higher melting point than fluorine because there are stronger intermolecular forces which need more energy to overcome
Give the charge of the ion formed when a halogen reacts with Group 1 metal.
-1
Why is fluorine the most reactive halogen?
It has the fewest shells so it easier for the nucleus to attract an electron
Explain why reactivity decreases going down Group 7
Reactivity decreases going down Group 7 because the atoms have more shells. This means that there is a less attraction between an incoming electron and the positive nucleus, which makes it harder to gain an electron
Where are the transition elements located in the Periodic Table
between Group 2 and Group 3
What are the typical properties of transition elements
High densities
High melting points
Form coloured compounds
Act as catalysts
Compare the hardness of transition metals to Group 1 metals
Transition metals are much harder than Group 1 metals which are very soft and light
How do the melting points of transition metals compare to those of Group 1 metals?
Transition metals have much higher melting points than Group 1 metals
How do Group 1 metals and transition metals differ in their reaction with oxygen?
Group 1 metals tarnish quickly in the presence of oxygen forming a metal oxide
Transition metals react much more slowly
What are two key characteristics that define a transition element?
They form coloured compounds
They have multiple oxidation states
Compare the reactivity of Group 1 metals and transition metals with water, oxygen and halogems
Group 1 metals react readily with water, oxygen, and halogens, while transition metals either react very slowly or do not react at all with these substances
