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Chemistry paper 1
Metallic bonding
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Cards (61)
What is the main structure of metals?
Metals consist of a
giant structure
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What happens to the electrons in the outer shell of metal atoms?
They are
delocalized
and free to move
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What holds the atoms together in metallic bonding?
Electrostatic attraction
between
ions
and electrons
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How strong is metallic bonding?
Metallic bonding is very
strong
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What types of compounds are held together by metallic bonding?
Metallic
alloys
and
compounds
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What do delocalized electrons in metallic bonds produce?
All the properties of
metals
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Why do metallic compounds have high melting and boiling points?
Strong
electrostatic forces
require lots of energy
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What state are most metallic compounds at room temperature?
Generally
solid
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Why are metals generally not soluble in water?
Due to their strong
metallic bonding
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Why are metals denser than non-metals?
Metal ions
are packed closely together
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What property allows metals to be hammered into sheets?
Malleability
due to sliding layers of
atoms
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How do delocalized electrons contribute to conductivity?
They carry
electrical current
and thermal energy
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What basic physical properties do all metals share?
Similar basic physical properties due to
metallic bonding
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Why don't non-metals exhibit the same properties as metals?
Non-metals lack
metallic bonding
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What types of structures do non-metals form?
A variety of
different
structures
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What are common characteristics of non-metals?
Dull,
brittle
, low
boiling points
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How do non-metals generally behave in terms of electrical conductivity?
They do not generally conduct
electricity
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How do metals and non-metals differ in chemical properties?
Non-metals
gain
electrons, metals
lose
electrons
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Where are non-metals typically found on the periodic table?
Top
and
right-hand side
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Where are metals typically found on the periodic table?
Bottom
and
left-hand side
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What is the typical state of non-metals at room temperature?
They are not generally
solids
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What is the significance of the outer shell of electrons in metals?
They are generally
under half-filled
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What is the significance of the outer shell of electrons in non-metals?
They are generally
over half-filled
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What is a humorous reference made about a metal on the bus?
A metal was the
conductor
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What is the metallic element mentioned in the study material?
Copper
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What is the term for the positive ions in metallic bonding?
Metal ions
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What is the role of delocalized electrons in metallic bonding?
They create a
'sea of electrons'
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What is the effect of strong electrostatic forces in metals?
They require lots of
energy
to break
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What happens to the layers of atoms in a pure metal?
They can
slide
over each other
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What is the significance of the term 'delocalized' in metallic bonding?
Electrons
are free to move around
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How does the structure of metals contribute to their properties?
Regular structure allows for
conductivity
and
malleability
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What is the relationship between metallic bonding and the properties of metals?
Metallic
bonding
explains
their
physical
properties
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What is the role of energy in breaking metallic bonds?
High
energy
is needed to break them
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How do the properties of metals differ from those of non-metals?
Metals are
conductive
, non-metals are not
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What is the significance of the periodic table's layout for metals and non-metals?
It shows their
different
locations
and
properties
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How does the arrangement of electrons affect the properties of metals?
Delocalized
electrons enhance conductivity and malleability
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What is the impact of metallic bonding on the physical state of metals?
It generally keeps them solid at
room temperature
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How do the properties of metals relate to their applications?
Properties like
conductivity
make them useful
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What is the significance of the term 'malleable' in relation to metals?
It
means
they
can
be
shaped
easily
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How does the presence of delocalized electrons affect the thermal properties of metals?
They allow metals to
conduct heat
effectively
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