EL.8 Flashcards
Group 1 and group 2 chemistry
Elements of which groups belong in the s block?
Group 1 and 2.
How does reactivity change as you go down group 1 and 2?
Elements become more reactive, the most reactive metals are found at the bottom of each group
What trend does the elements in group 1 and 2 show in terms of becoming ions?
As you go down the groups, elements lose electrons easier and form cations more readily in ionic compounds. These elements are said to become more metallic as you go down the groups.
How does reactivity change as you move across the periodic table from the left to the right in terms of from group 1 to group 2?
They become less reactive. Group 1 metals are more reactive than group 2 metals in the same period. These elements are said to become less metallic as you move across the periods.
What are some descriptions for the physical properties of the s block metals?
They tend to be soft , weak metals with low melting points.
What reactions of s block metal make them not so useful in daily life?
They are too reactive with oxygen and water to become oxides and hydroxides.
How are group 1 and 2 metals normally found?
In compounds with other elements, they are never naturally found in their elemental form.
In group 1 and 2, elements show similarities in their reactions with elements in their group, and differences are also observed in groups as trends. What features about elements in the same group can be used to explain the similarities, and what can explain the differences?
Similarities of elements in the same group happen because of their similar arrangement of electrons in their atoms. The differences, on the other hand, happen because the size of atom increases down the group.
What does ionization mean?
The process of removing or adding an electron to an atom so it becomes an ion.
What is the energy required to remove one electron from an atom known as?
First ionization enthalpy
What is the general equation for the first ionization process?
X(g) → X+(g) + e-
What are some conditions to be included when stating the first ionization enthalpy of an element?
It is the amount of energy required to remove one electron from one mole of atoms of that element in its gaseous form.
Which electron would be removed in first ionization?
The most loosely held electron, this will be one of the outer shell electrons.
Elements from which group have the highest first ionization enthalpies?
Group 0, noble gases, they are extremely stable and very difficult to ionize.
Elements from which group have the lowest first ionization enthalpies?
Group 1, with only one outer shell electron, they are very reactive and very easy to ionize.
What is the general trend in first ionization enthalpy across a period and what is the reason for this trend?
As you go across a period, it becomes more difficult to remove an electron, the ionization enthalpy show a general increase. This is because as electrons are being added to the outer shell, protons are being added to the nucleus too. And as the nuclear charge becomes more positive, electrons in the outer shell are held more tightly, making them more difficult to remove going across a period.
