1 - Elements of Life (EL) Flashcards by Nico Walker

What other group has similar properties to group 2?

Group 1

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Describe the reactivity of group 2 hydroxides

Increases going down the periodic table (Calcium Hydroxide is least reactive)

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Describe the reactivity of group 2 sulfates

Decreases going down the periodic table (Barium Sulfate is least reactive)

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Describe the trend of ionisation energy in group 2

Decreases down group
- Less electrostatic attraction
-Outermost shell is further from the nucleus

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Describe the trend of reactivity in group 2 metals

Increases down the group - outermost shell gets further away from nucleus

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Describe the trend of melting points in group 2 metals

Decreases down group

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Describe thermal stability of group 2 carbonates

Increases down group
-Depends on charge density
-Smaller ion = higher charge density
-Higher charge density = less thermal stability, more CO3 distortion (products: CO2 and O2-) and forms more moles of carbonate

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What is a spectrometer?

A machine that works out the atomic mass and formula mass of a sample

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1st stage of spectrometry

Injection
-sample injected

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2nd stage of spectrometry

Vaporisation
-sample heated to a gas

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3rd stage of spectrometry

Ionisation chamber
-hit with high energy electrons - turns into cations

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4th stage of spectrometry

Acceleration area
-ions accelerated to same KE as an electric field

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5th Stage of spectrometry

Drift region
-ions travel through magnetic field

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6th stage of spectrometry

Detector
-time to reach detector is measured
-cations gain electrons and create current

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What does the current created say about the number of ions?

High = lots of ions

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What does the speed that the ions hit the detector show?

Slow speed = heavier ions

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Define periodicity

Regular variation of properties of elements with their position in the periodic table

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What is first ionisation energy?

Energy required to remove 1 mole of electrons from 1 mole of a gaseous element
Example: Na(g) –> Na+(g) + e-

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Why is ionisation energy always measured in gaseous state?

Eliminates energy for melting/boiling

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Trend of atomic radius in period 3

-Electrons added to same shell
-More protons in nucleus, stronger attraction between nucleus and outermost shell
-Atomic radius decreases

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Trend of melting/boiling points in period 3

Starts high - giant metallic and covalent structures
Then decreases - simple covalent

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Define successive ionisation energy

A measure of the energy required to remove 1 mole of electrons in turn from 1 mole of gaseous atoms/ions

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Define energy (/shell) level

Electrons at the same energy level are in the same shell
(Number)

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Define sub shell

Within a shell. Successive subshells have extra subshells
(Letter)

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Define orbital

Region of space where 2 electrons spend 98% of their time. Within a subshell (Boxes/superscript numbers)

What are the orbitals?

1 s-orbital 3 p-orbitals 5 d-orbitals

Shape of an s-orbital?

Spherical

Shape of a p-orbital?

Dumbell (drawn like figure of 8 on xyz-axis) Can be any orientation

Shape of a d-orbital?

Various shapes and orientation

How many s-orbitals are in each electron shell?

How many p-orbitals are in each electron shell?

3, from 2nd shell onward

How many d-orbitals are in each electron shell?

5, from 2nd shell onward

Full electron configuration of potassium?

1s2 2s2 3p6 3s2 3p6 4s1

Noble gas configuration of potassium?

[Ar] 4s1

What is VESPR theory?

Explains the shape of electrons based on the number of ares of electron density around the central atom

Considered points in VESPR theory

-Central atom -Number of areas of electron density (bonds and lone pairs) -Electrons repel as far as possible (AFAP) -Lone pairs repel more than bonding pairs

Define dative covalent bond

A covalent bond where both electrons are supplied by one bonding atom

Bond angle for 2 areas of electron density

180°

Bond angle for 3 areas of electron density

120°

Bond angle for 4 areas of electron density

109.5°

Bond angle for 5 areas of electron density

120° and 90°

Bond angle for 6 areas of electron density

90°

Shape for 2 areas of electron density

Linear

Shape for 3 areas of electron density

Trigonal Planar

Shape for 4 areas of electron density

Tetrahedral

Shape for 5 areas of electron density

Trigonal bipyramidal

Shape for 6 areas of electron density

Octahedral

What does a wedge mean in drawing VESPR?

Drawing coming out infront of paper plane

What does a dashed line mean in drawing VESPR?

Drawing going behind the plane of paper

Drawing for 4 areas of electron density

2 normal lines 1 wedge 1 dashed line

Drawing for 5 areas of electron density

3 normal lines 1 wedge 1 dashed line 90° between 2 normal lines 120° between middle normal and wedge

Drawing for 6 areas of electron density

4 normal lines 1 wedge 1 dashed line

Bond angle for 4 areas of electron density with 1 lone pair

107°

Bond angle for 4 areas of electron density with 2 lone pairs

104.5°

Shape for 4 areas of electron density with 1 lone pair

Trigonal pyramidal

Shape for 4 areas of electron density with 2 lone pairs

(Linear) bent

Drawing for 4 areas of electron density with 1 lone pair

1 normal line 1 wedge 1 dashed line

Drawing for 4 areas of electron density with 2 lone pairs

2 normal lines

What colour do copper ions go when burnt?

Blue-green

What colour do lithium ions go when burnt?

Crimson

What colour do potassium ions go when burnt?

Lilac

What colour do sodium ions go when burnt?

Yellow

What colour do calcium ions go when burnt?

Brick red

What colour do barium ions go when burnt?

Green

What colour precipitate is formed when copper (II) reacts with NaOH?

Blue

What colour precipitate is formed when iron (II) reacts with NaOH?

Green

What colour precipitate is formed when iron (III) reacts with NaOH?

Brown

What colour precipitate is formed when calcium ions react with NaOH?

White

What colour precipitate is formed when aluminum ions react with NH4OH?

White

What colour precipitate is formed when zinc (II) ions react with NH4OH?

White

What happens if excess NH4OH is added to zinc (II) ions?

Redissolves into a colourless solution

What is used to test for lead (II) ions?

Potassium iodide

What colour is the precipitate for a positive test for lead (II) ions?

Yellow

What is used to test for sulfate ions?

Barium chloride

What colour is the precipitate for a positive test for sulfate ions?

White

What is used to test the halide ions?

Silver nitrate

What colour is the precipitate for a positive test for chloride ions?

White

What colour is the precipitate for a positive test for bromide ions?

Cream

What colour is the precipitate for a positive test for iodide ions?

Yellow

What is used to test ammonium ions?

Sodium hydroxide

What is used to test nitrate ions?

Sodium hydroxide and aluminum

How can the ammonia formed be tested?

Damp red litmus paper would be turned blue

What is the result for a positive test for ammonium/nitrate ions?

When warmed ammonia is formed

What is used to test for carbonate ions?

Acid

What gas would form in a positive test for carbonate ions?

CO2

How can the gas in the test for carbonate ions be tested?

Bubble gas through limewater. If CO2 present then limewater will go from clear to cloudy

Define excited electron state

Electron placement after energy absorption

Define ground electron state

Where electrons are normally

What does an absorption spectra look like?

-Coloured background -Black lines -Lines get closer at higher frequencies

What does an emission spectra look like?

-Black background -Coloured lines -Lines get closer at higher frequencies

Why do the lines on absorption/emission spectra get closer at higher frequencies?

Energy levels decrease further from an atom's nucleus

What are the products formed when a metal and acid are reacted?

Salt and hydrogen

What are the products formed when a metal hydroxide and acid are reacted?

Salt and water

What are the products formed when a metal oxide and acid are reacted?

Salt and water

What are the products formed when a metal carbonate and acid are reacted?

Salt, water and carbon dioxide

How are insoluble salts made?

-Make precipitate from 2 soluble salts -Filter -Rinse in distilled water -Dry

How are soluble salts made using metals/insoluble bases?

-Add solid in excess -Filter -Heat solution -Pat dry

How are soluble salts made using acids and alkalis?

-Do a titration and using indicator -Note the volumes for neutralisation -Repeat using exact values (no indicator) -Heat solution -Pat dry

Equation with Planck’s constant and frequency

E = hv E - Energy/J h - Planck’s constant/J Hz^-1 v - Frequency/Hz

Equation with Planck’s constant and wavelength

E = hc/λ E - Energy/J h - Planck’s constant/J Hz^-1 c - Speed of light/m s^-1 λ - Wavelength/m