BTEC Applied Science Unit Chemistry (correct answers)
How many electrons can an s subshell hold? correct answers 2
How many electrons can a p subshell hold? correct answers 6
How many electrons can a d subshell hold? correct answers 10
Which subshells are available in the first energy level? correct answers s
Which subshells are available in the second energy level? correct answers s and p
Which subshells are available in the third energy level? correct answers s, p and d
What is Hund's rule? correct answers Orbitals must all be singly filled before they can
be doubly occupied
Which elements do not fill the 4s subshell before the 3d subshell? correct answers
Copper and chromium
Define the term ionic bond correct answers The electrostatic attraction between
oppositely charged ions
What is the charge of an ion from group 1? correct answers +1
What is the charge of an ion from group 2? correct answers +2
What is the charge of an ion from group 6? correct answers -2
What is the charge of an ion from group 7? correct answers -1
Explain how atoms of sodium react with atoms of chlorine correct answers Na loses its
2s1 electron gaining a +ve charge.
Cl gains an electron in the 3p subshell gaining a -ve charge.
The opposite charges attract to form NaCl
Why do ionic bonds have such high melting points? correct answers Each +ve ion is
surrounded by 6 -ve ions and vice versa.
Strong electrostatic attraction in every direction.
Requires a large amount of energy to break
State two factors that affect the strength of an ionic bond correct answers Size of ion
and charge on ion
When can ionic substances conduct electricity? correct answers When molten or in
aqueous solution
,Describe the properties of ionic compounds correct answers Conduct electricity when
molten or aqueous solution
High melting/boiling points
Usually soluble in water
Define the term covalent bond correct answers A shared pair of electrons
Which metals lose electrons from the 4s subshell before the 3d subshell? correct
answers Transition metals
Why do metals have such high melting points? correct answers Strong force of
attraction between positive ions and delocalised electrons. This requires a large amount
of energy to overcome.
State the two factors that affect the strength of metallic bonding correct answers Size of
ion
Charge on ion
Explain how the charge on metal ions affects the strength of the metallic bond correct
answers The larger the +ve charge the greater the attraction between the nucleus and
the delocalised electrons
Explain how the size of the metal ions affects the strength of the metallic bond correct
answers The smaller the +ve ion the closer the nucleus is to the delocalised electrons
creating a greater attraction
Explain why metals conduct electricity correct answers The delocalised electrons 'carry'
charge. Current flows because of this.
Explain why metals conduct heat correct answers Particles are paced tightly so kinetic
energy is passed from ion to ion. The delocalised electrons also enable heat to be
passed.
Explain why metals are ductile and malleable correct answers The lattice structure
allows layers of metal ions to slide over each other without disrupting bonding
Name the 3 forces between molecules correct answers Van der Waals
Permanent dipole-dipole
Hydrogen bonds
Order the 3 forces between molecules in order of strongest to weakest correct answers
Hydrogen bonds
Permanent dipole-dipole
Van der Waals
, How are Van der Waal's forces formed? correct answers Electrons move to one side,
caused temporary dipole. This induces a temporary dipole in neighbouring molecules.
Attraction occurs between oppositely charged dipoles
In what molecules do Van der Waal's forces exist? correct answers Non-polar
molecules
How are permanent dipole-dipole forces formed? correct answers Permanent dipole in
one molecule attracts oppositely charged permanent dipole in neighbouring molecule
In which molecules do permanent dipole-dipole forces exist? correct answers Polar
molecules
Which elements must be present for hydrogen bonds to exist? correct answers
Hydrogen and either nitrogen, oxygen or fluorine
What is meant by the term displacement? correct answers When a more reactive
element takes the place of a less reactive element in a compound
State the equation for determining moles correct answers Moles = mass ÷ relative
atomic mass (molar mass)
Define the term Avogadro's Constant correct answers The number of atoms in a mole of
a given substance. Quoted as 6.02x10^23
Define the term relative atomic mass correct answers The average mass of an atom of
an element relative to 1/12th the relative atomic mass of Carbon12
Define the term relative molecular mass correct answers The average mass of a
molecule relative to 1/12th the relative atomic mass of Carbon12
What does this number represent? 6.02x10^23 correct answers The number of particles
in a mole. Commonly called Avogadro's Constant
What is the equation for calculating % yield? correct answers % yield = (actual yield ÷
theoretical yield) x 100
What groups are included in the 's' block of the periodic table? correct answers Groups
1 and 2
What part of the periodic table is known as the 'd' block? correct answers Transition
metals
Which groups are in the 'p' block of the periodic table? correct answers 3, 4, 5, 6 and 7
What is a group on the periodic table? correct answers A vertical column
How many electrons can an s subshell hold? correct answers 2
How many electrons can a p subshell hold? correct answers 6
How many electrons can a d subshell hold? correct answers 10
Which subshells are available in the first energy level? correct answers s
Which subshells are available in the second energy level? correct answers s and p
Which subshells are available in the third energy level? correct answers s, p and d
What is Hund's rule? correct answers Orbitals must all be singly filled before they can
be doubly occupied
Which elements do not fill the 4s subshell before the 3d subshell? correct answers
Copper and chromium
Define the term ionic bond correct answers The electrostatic attraction between
oppositely charged ions
What is the charge of an ion from group 1? correct answers +1
What is the charge of an ion from group 2? correct answers +2
What is the charge of an ion from group 6? correct answers -2
What is the charge of an ion from group 7? correct answers -1
Explain how atoms of sodium react with atoms of chlorine correct answers Na loses its
2s1 electron gaining a +ve charge.
Cl gains an electron in the 3p subshell gaining a -ve charge.
The opposite charges attract to form NaCl
Why do ionic bonds have such high melting points? correct answers Each +ve ion is
surrounded by 6 -ve ions and vice versa.
Strong electrostatic attraction in every direction.
Requires a large amount of energy to break
State two factors that affect the strength of an ionic bond correct answers Size of ion
and charge on ion
When can ionic substances conduct electricity? correct answers When molten or in
aqueous solution
,Describe the properties of ionic compounds correct answers Conduct electricity when
molten or aqueous solution
High melting/boiling points
Usually soluble in water
Define the term covalent bond correct answers A shared pair of electrons
Which metals lose electrons from the 4s subshell before the 3d subshell? correct
answers Transition metals
Why do metals have such high melting points? correct answers Strong force of
attraction between positive ions and delocalised electrons. This requires a large amount
of energy to overcome.
State the two factors that affect the strength of metallic bonding correct answers Size of
ion
Charge on ion
Explain how the charge on metal ions affects the strength of the metallic bond correct
answers The larger the +ve charge the greater the attraction between the nucleus and
the delocalised electrons
Explain how the size of the metal ions affects the strength of the metallic bond correct
answers The smaller the +ve ion the closer the nucleus is to the delocalised electrons
creating a greater attraction
Explain why metals conduct electricity correct answers The delocalised electrons 'carry'
charge. Current flows because of this.
Explain why metals conduct heat correct answers Particles are paced tightly so kinetic
energy is passed from ion to ion. The delocalised electrons also enable heat to be
passed.
Explain why metals are ductile and malleable correct answers The lattice structure
allows layers of metal ions to slide over each other without disrupting bonding
Name the 3 forces between molecules correct answers Van der Waals
Permanent dipole-dipole
Hydrogen bonds
Order the 3 forces between molecules in order of strongest to weakest correct answers
Hydrogen bonds
Permanent dipole-dipole
Van der Waals
, How are Van der Waal's forces formed? correct answers Electrons move to one side,
caused temporary dipole. This induces a temporary dipole in neighbouring molecules.
Attraction occurs between oppositely charged dipoles
In what molecules do Van der Waal's forces exist? correct answers Non-polar
molecules
How are permanent dipole-dipole forces formed? correct answers Permanent dipole in
one molecule attracts oppositely charged permanent dipole in neighbouring molecule
In which molecules do permanent dipole-dipole forces exist? correct answers Polar
molecules
Which elements must be present for hydrogen bonds to exist? correct answers
Hydrogen and either nitrogen, oxygen or fluorine
What is meant by the term displacement? correct answers When a more reactive
element takes the place of a less reactive element in a compound
State the equation for determining moles correct answers Moles = mass ÷ relative
atomic mass (molar mass)
Define the term Avogadro's Constant correct answers The number of atoms in a mole of
a given substance. Quoted as 6.02x10^23
Define the term relative atomic mass correct answers The average mass of an atom of
an element relative to 1/12th the relative atomic mass of Carbon12
Define the term relative molecular mass correct answers The average mass of a
molecule relative to 1/12th the relative atomic mass of Carbon12
What does this number represent? 6.02x10^23 correct answers The number of particles
in a mole. Commonly called Avogadro's Constant
What is the equation for calculating % yield? correct answers % yield = (actual yield ÷
theoretical yield) x 100
What groups are included in the 's' block of the periodic table? correct answers Groups
1 and 2
What part of the periodic table is known as the 'd' block? correct answers Transition
metals
Which groups are in the 'p' block of the periodic table? correct answers 3, 4, 5, 6 and 7
What is a group on the periodic table? correct answers A vertical column
