Why do different isotopes of the same element have the same chemical properties?
The number of electrons in the outer shell is the same (electrons are involved in chemical reactions)
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State and explain two anomalous properties of ice caused by hydrogen bonding
Ice is less dense than water due to molecules arranging in an open lattice structure. Has a relatively high melting point due to relatively strong hydrogen bonds.
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Describe and explain the electrical conductivity of sodium oxide and sodium in solid and molten states.
Sodium oxide = giant ionic lattice so cannot conduct when solid as ions are in fixed positions but can when molten as ions are mobile. Sodium can conduct as a solid and molten due to delocalised electrons.
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State and explain the trend in atomic radius from Li to F
Atomic radius decreases from Li to F because nuclear charge increases but electrons are being added to the same shell so experience the same shielding. Outer electrons are more attracted to the +ve nucleus so the outer shell is drawn in slightly.
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Which group 2 carbonate decomposes at the highest temperature?
RaCO3
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How is a salt formed?
A hydrogen ion in an acid is replaced by a metal ion
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What is meant by empirical formula?
The simplest whole number ratio of atoms present in a compound
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Describe what is meant by an ionic lattice in terms of type and arrangement of particles present
Oppositely charged ions held by ionic bonds in a repeating pattern
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Chlorine gas can be added to a cold, dilute alkaline solution to form bleach. What is the equation?
Explain how and why the attraction between nuclei in outermost electrons in gaseous atoms varies across period 3.
The attraction between nuclei and outermost electrons increases across period 3 because the nuclear charge increases but electrons are being added to the same shell so the outer shell is drawn inwards slightly = atomic radius decreases.
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Explain the different boiling points between NH3 (-33), F2 (-188) and Br2 (+59)
Ammonia has hydrogen bonding (due to permanent dipole). F2 and Br2 both display Van der Waals forces due to random oscillations of electrons (simple molecular) but they're stronger in Br2 due to having more electrons and stronger than H-bonds.
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Other cards in this set
Card 2
Front
State and explain two anomalous properties of ice caused by hydrogen bonding
Back
Ice is less dense than water due to molecules arranging in an open lattice structure. Has a relatively high melting point due to relatively strong hydrogen bonds.
Card 3
Front
Describe and explain the electrical conductivity of sodium oxide and sodium in solid and molten states.
Back
Card 4
Front
State and explain the trend in atomic radius from Li to F
Back
Card 5
Front
Which group 2 carbonate decomposes at the highest temperature?
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