BTEC Applied Science Unit 1 Chemistry
How many electrons can an s subshell hold? correct answer2
How many electrons can a p subshell hold? correct answer6
How many electrons can a d subshell hold? correct answer10
Which subshells are available in the first energy level? correct answers
Which subshells are available in the second energy level? correct answers and p
Which subshells are available in the third energy level? correct answers, p and d
What is Hund's rule? correct answerOrbitals must all be singly filled before they can be doubly occupied
Which elements do not fill the 4s subshell before the 3d subshell? correct answerCopper and chromium
Define the term ionic bond correct answerThe electrostatic attraction between oppositely charged ions
What is the charge of an ion from group 1? correct answer+1
What is the charge of an ion from group 2? correct answer+2
,What is the charge of an ion from group 6? correct answer-2
What is the charge of an ion from group 7? correct answer-1
Explain how atoms of sodium react with atoms of chlorine correct answerNa 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 answerEach +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 answerSize of ion and charge on ion
When can ionic substances conduct electricity? correct answerWhen molten or in aqueous solution
Describe the properties of ionic compounds correct answerConduct electricity when molten or aqueous
solution
High melting/boiling points
Usually soluble in water
Define the term covalent bond correct answerA shared pair of electrons
Which metals lose electrons from the 4s subshell before the 3d subshell? correct answerTransition
metals
, Why do metals have such high melting points? correct answerStrong 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 answerSize of ion
Charge on ion
Explain how the charge on metal ions affects the strength of the metallic bond correct answerThe 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 answerThe
smaller the +ve ion the closer the nucleus is to the delocalised electrons creating a greater attraction
Explain why metals conduct electricity correct answerThe delocalised electrons 'carry' charge. Current
flows because of this.
Explain why metals conduct heat correct answerParticles 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 answerThe lattice structure allows layers of metal
ions to slide over each other without disrupting bonding
Name the 3 forces between molecules correct answerVan der Waals
Permanent dipole-dipole
Hydrogen bonds
Order the 3 forces between molecules in order of strongest to weakest correct answerHydrogen bonds
Permanent dipole-dipole
How many electrons can an s subshell hold? correct answer2
How many electrons can a p subshell hold? correct answer6
How many electrons can a d subshell hold? correct answer10
Which subshells are available in the first energy level? correct answers
Which subshells are available in the second energy level? correct answers and p
Which subshells are available in the third energy level? correct answers, p and d
What is Hund's rule? correct answerOrbitals must all be singly filled before they can be doubly occupied
Which elements do not fill the 4s subshell before the 3d subshell? correct answerCopper and chromium
Define the term ionic bond correct answerThe electrostatic attraction between oppositely charged ions
What is the charge of an ion from group 1? correct answer+1
What is the charge of an ion from group 2? correct answer+2
,What is the charge of an ion from group 6? correct answer-2
What is the charge of an ion from group 7? correct answer-1
Explain how atoms of sodium react with atoms of chlorine correct answerNa 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 answerEach +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 answerSize of ion and charge on ion
When can ionic substances conduct electricity? correct answerWhen molten or in aqueous solution
Describe the properties of ionic compounds correct answerConduct electricity when molten or aqueous
solution
High melting/boiling points
Usually soluble in water
Define the term covalent bond correct answerA shared pair of electrons
Which metals lose electrons from the 4s subshell before the 3d subshell? correct answerTransition
metals
, Why do metals have such high melting points? correct answerStrong 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 answerSize of ion
Charge on ion
Explain how the charge on metal ions affects the strength of the metallic bond correct answerThe 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 answerThe
smaller the +ve ion the closer the nucleus is to the delocalised electrons creating a greater attraction
Explain why metals conduct electricity correct answerThe delocalised electrons 'carry' charge. Current
flows because of this.
Explain why metals conduct heat correct answerParticles 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 answerThe lattice structure allows layers of metal
ions to slide over each other without disrupting bonding
Name the 3 forces between molecules correct answerVan der Waals
Permanent dipole-dipole
Hydrogen bonds
Order the 3 forces between molecules in order of strongest to weakest correct answerHydrogen bonds
Permanent dipole-dipole
