3/22/25, 11:54 BTEC Applied Science All Flashcards |
AM
BTEC APPLIED SCIENCE ALL EXAM QUESTIONS AND ANSWERS
WITH COMPLETE SOLUTIONS VERIFIED LATEST UPDATE
Terms in this set (221)
How many electrons can an s subshell 2
hold?
How many electrons can a p subshell hold? 6
How many electrons can a d subshell hold? 10
What is Hund's rule? Orbitals must all be singly filled before they can be doubly occupied
Define the term ionic bond The electrostatic attraction between oppositely charged ions
What is the charge of an ion from group 1? +1
What is the charge of an ion from group 2? +2
What is the charge of an ion from group 6? -2
What is the charge of an ion from group 7? -1
Na loses its 2s1 electron gaining a +ve charge.
Explain how atoms of sodium react with
Cl gains an electron in the 3p subshell gaining a -ve charge.
atoms of chlorine
The opposite charges attract to form NaCl
Each +ve ion is surrounded by 6 -ve ions and vice versa.
Why do ionic bonds have such high melting
Strong electrostatic attraction in every direction.
points?
Requires a large amount of energy to break
State two factors that affect the strength Size of ion and charge on ion
of an ionic bond
When can ionic substances conduct When molten or in aqueous solution
electricity?
Conduct electricity when molten or aqueous solution
Describe the properties of ionic
High melting/boiling points
compounds
Usually soluble in water
Define the term covalent bond A shared pair of electrons
Which metals lose electrons from the 4s Transition metals
subshell before the 3d subshell?
Why do metals have such high melting Strong force of attraction between positive ions and delocalised electrons. This
points? requires a large amount of energy to overcome.
State the two factors that affect the Size of ion
strength of metallic bonding Charge on ion
Explain how the charge on metal ions The larger the +ve charge the greater the attraction between the nucleus and the
affects the strength of the metallic bond delocalised electrons
Explain how the size of the metal ions The smaller the +ve ion the closer the nucleus is to the delocalised electrons
affects the strength of the metallic bond creating a greater attraction
Explain why metals conduct electricity The delocalised electrons 'carry' charge. Current flows because of this.
Particles are paced tightly so kinetic energy is passed from ion to ion. The
Explain why metals conduct heat
delocalised electrons also enable heat to be passed.
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5
, 3/22/25, 11:54 BTEC Applied Science All Flashcards |
AM
Explain why metals are ductile and The lattice structure allows layers of metal ions to slide over each other without
malleable disrupting bonding
Van der Waals
Name the 3 forces between molecules Permanent dipole-
dipole Hydrogen bonds
Hydrogen bonds
Order the 3 forces between molecules in
Permanent dipole-
order of strongest to weakest
dipole Van der Waals
Electrons move to one side, caused temporary dipole. This induces a temporary
How are Van der Waal's forces formed? dipole in neighbouring molecules. Attraction occurs between oppositely charged
dipoles
In what molecules do Van der Waal's forces Non-polar molecules
exist?
How are permanent dipole-dipole forces Permanent dipole in one molecule attracts oppositely charged permanent dipole in
formed? neighbouring molecule
In which molecules do permanent dipole- Polar molecules
dipole forces exist?
Which elements must be present for Hydrogen and either nitrogen, oxygen or fluorine
hydrogen bonds to exist?
When a more reactive element takes the place of a less reactive element in a
What is meant by the term displacement?
compound
Moles = mass ÷ relative atomic mass (molar mass)
State the equation for determining moles
(Mass= mr X moles)
Define the term Avogadro's Constant The number of atoms in a mole of a given substance
What is the equation for calculating % yield = (actual yield ÷ theoretical yield) x 100
% yield?
What is a group on the periodic table? A vertical column
What is a period on the periodic table? A horizontal row
The energy required to remove the outermost electron from one mole of gaseous
Define the term first ionisation energy
atoms to produce one mole of gaseous +1 ions
Define the term atomic radius The distance between the nucleus of an atom and the outermost electron
A measure of how well an atom attracts a bonding pair of electrons in a covalent
Define the term electronegativity
bond
Define the term malleability How easily a material can be hammered into shape
Define the term ductility How easily a material can be drawn into wires
Describe the trend in atomic radius down Atomic radius increases
any group
Explain the trend in atomic radius down Higher energy levels are filled. The orbitals in higher energy levels are further from
any group the nucleus
Describe the trend in first ionisation energy First ionisation energy decreases
down groups 1 and 2
Increased electron shielding
Explain the trend in first ionisation energy Greater atomic radius
down groups 1 and 2 Smaller attraction to +ve nucleus
SO electron is easier to remove requiring less energy
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5
AM
BTEC APPLIED SCIENCE ALL EXAM QUESTIONS AND ANSWERS
WITH COMPLETE SOLUTIONS VERIFIED LATEST UPDATE
Terms in this set (221)
How many electrons can an s subshell 2
hold?
How many electrons can a p subshell hold? 6
How many electrons can a d subshell hold? 10
What is Hund's rule? Orbitals must all be singly filled before they can be doubly occupied
Define the term ionic bond The electrostatic attraction between oppositely charged ions
What is the charge of an ion from group 1? +1
What is the charge of an ion from group 2? +2
What is the charge of an ion from group 6? -2
What is the charge of an ion from group 7? -1
Na loses its 2s1 electron gaining a +ve charge.
Explain how atoms of sodium react with
Cl gains an electron in the 3p subshell gaining a -ve charge.
atoms of chlorine
The opposite charges attract to form NaCl
Each +ve ion is surrounded by 6 -ve ions and vice versa.
Why do ionic bonds have such high melting
Strong electrostatic attraction in every direction.
points?
Requires a large amount of energy to break
State two factors that affect the strength Size of ion and charge on ion
of an ionic bond
When can ionic substances conduct When molten or in aqueous solution
electricity?
Conduct electricity when molten or aqueous solution
Describe the properties of ionic
High melting/boiling points
compounds
Usually soluble in water
Define the term covalent bond A shared pair of electrons
Which metals lose electrons from the 4s Transition metals
subshell before the 3d subshell?
Why do metals have such high melting Strong force of attraction between positive ions and delocalised electrons. This
points? requires a large amount of energy to overcome.
State the two factors that affect the Size of ion
strength of metallic bonding Charge on ion
Explain how the charge on metal ions The larger the +ve charge the greater the attraction between the nucleus and the
affects the strength of the metallic bond delocalised electrons
Explain how the size of the metal ions The smaller the +ve ion the closer the nucleus is to the delocalised electrons
affects the strength of the metallic bond creating a greater attraction
Explain why metals conduct electricity The delocalised electrons 'carry' charge. Current flows because of this.
Particles are paced tightly so kinetic energy is passed from ion to ion. The
Explain why metals conduct heat
delocalised electrons also enable heat to be passed.
1/
5
, 3/22/25, 11:54 BTEC Applied Science All Flashcards |
AM
Explain why metals are ductile and The lattice structure allows layers of metal ions to slide over each other without
malleable disrupting bonding
Van der Waals
Name the 3 forces between molecules Permanent dipole-
dipole Hydrogen bonds
Hydrogen bonds
Order the 3 forces between molecules in
Permanent dipole-
order of strongest to weakest
dipole Van der Waals
Electrons move to one side, caused temporary dipole. This induces a temporary
How are Van der Waal's forces formed? dipole in neighbouring molecules. Attraction occurs between oppositely charged
dipoles
In what molecules do Van der Waal's forces Non-polar molecules
exist?
How are permanent dipole-dipole forces Permanent dipole in one molecule attracts oppositely charged permanent dipole in
formed? neighbouring molecule
In which molecules do permanent dipole- Polar molecules
dipole forces exist?
Which elements must be present for Hydrogen and either nitrogen, oxygen or fluorine
hydrogen bonds to exist?
When a more reactive element takes the place of a less reactive element in a
What is meant by the term displacement?
compound
Moles = mass ÷ relative atomic mass (molar mass)
State the equation for determining moles
(Mass= mr X moles)
Define the term Avogadro's Constant The number of atoms in a mole of a given substance
What is the equation for calculating % yield = (actual yield ÷ theoretical yield) x 100
% yield?
What is a group on the periodic table? A vertical column
What is a period on the periodic table? A horizontal row
The energy required to remove the outermost electron from one mole of gaseous
Define the term first ionisation energy
atoms to produce one mole of gaseous +1 ions
Define the term atomic radius The distance between the nucleus of an atom and the outermost electron
A measure of how well an atom attracts a bonding pair of electrons in a covalent
Define the term electronegativity
bond
Define the term malleability How easily a material can be hammered into shape
Define the term ductility How easily a material can be drawn into wires
Describe the trend in atomic radius down Atomic radius increases
any group
Explain the trend in atomic radius down Higher energy levels are filled. The orbitals in higher energy levels are further from
any group the nucleus
Describe the trend in first ionisation energy First ionisation energy decreases
down groups 1 and 2
Increased electron shielding
Explain the trend in first ionisation energy Greater atomic radius
down groups 1 and 2 Smaller attraction to +ve nucleus
SO electron is easier to remove requiring less energy
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