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Chemistry > Module 2 Foundations in Chemistry > Flashcards

Module 2 Foundations in Chemistry Flashcards

1
Q

How does a temporary dipole dipole interaction occur

A

2 Non - Polar molecules creates an instantaneous dipoe
This induces a dipole in an atom
The attraction between 2 dipoles is called an LDF

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2
Q

What 3 elements form Hydrogen Bonds and why

A

Fluorine, Chlorine and Iodine as they’re very electronegative

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3
Q

What is different about compounds with Hydrogen Bonds

A

They’re solube in water due to -OH bonds and their melting points are higher than normal molecules and ice is less dense than water due to molecules in ice is held apart by Hydrogen Bonds

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4
Q

What is a linear atom nd what is the angle

A

2BP 0 LP –> 180 degrees

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5
Q

What is a triganol planar molecule and what is the angle?

A

3BP 0 LP Angle - 120degrees

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6
Q

What is a tetrahedral molecule and what is the angle

A

4BP O LP Angle - 109.5 degrees

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7
Q

What is a triganol byprimdal molecule and what is the angle

A

5BP 0LP Angle 2 is 90 3 is 109.5

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8
Q

What happens to the bond angle everytime a LP Is added

A

Decreases by 2.5degrees

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9
Q

What is the name for each LP added after tetrahedral

A

Tetrahedral – Triganol Pyrimidal – Non- Linear

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10
Q

What 3 atoms form dative covalent bonds

A

Boron TriFluoride, ammonium and carbon monoxide

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11
Q

What is special about Born Trifluoride

A

It only has 6 electrons in the outer shell

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12
Q

What is the defentiion of electronegativity

A

The ability of atoms to attract bonding pair of electrons in a covalent bond

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13
Q

What is the trend of electronegativity across a periodic table

A

More electronegative up the table as smaller radisu and more electronegative across the table as there is a larger nuclear charge

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14
Q

What do polar molecules have

A

An Overall Dipole

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15
Q

What happens to symmetrical atoms

A

They cancel eachother out so there is no overall dipole

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16
Q

What are the ion charges for:
Sulfate
Nitrate
Carbonate
Phosphate
Ammonium

A

SO4 2-
CO3 2-
NO3 -
PO4 3-
NH4 +

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17
Q

What are the defenitions for:
Relative atomic mass

A

Weighted mean mass of an atom of an element compared to 1/12th the mass of C-12

18
Q

What is the defenition of relative isotopic mass

A

Mass of an atom of an isotope of an element compared to 1-12th the mass of C-12

19
Q

Defenition of molecular mass

A

The average mass of a moleucle compared to 1-12th the mass of C-12

20
Q

Defenition of relative formula mass

A

The average mass of a formula unit compared to 1-12th the mass of C-12

21
Q

Formula for ideal gases and conversion units

A

pV = nRT
P = pressure in Pa (x1000 if kPA)
V = vol in m^3
n = mol.
R = 8.314
T = in K. ( add 273)

22
Q

What is 1 atm. in pa

A

100,000 Pa

23
Q

What are the 2 formulas for conc.

A

Mol / vol
Mass / vol

24
Q

What is the formula for dilution

A

C1V1 = C2V2

25
Q

What is the defenition for emperical formula

A

Simplest whole number ratio of atoms of each element present in a compound

26
Q

Why is it good to have a high atom economy

A

Little to no waste products and the process is more economcially viable ahd helps to preserve raw materials

27
Q

How would you:
Measure mass
Measure vol. of a solution
Measure gas produced in a reaction

A

Mass –> Use a digital mass balance - use balance with suitable resolution

Vol. for a solution –> Measure vol. of a solution and if making up standard solution, use volumetric flask for required vol.

Gas produced –> Gas Syringe

27
Q

What is an acid and alkali

A

Acid –> Proton Donor
Alkali –> Proton Acceptor

28
Q

What is the defenition of strong and weak acid

A

Strong –> Fully dissasociates in aqueous solution
Weak —> Partially dissasosicates in aqeuous solution

29
Q

What are the reations of acids with bases

A

Acid + Carbomate –> Salt + Water + Carbon Dioxide

Acid + Metal Oxide –> Salt + Water

Metal + Acid –> Salt + Hydrogen

30
Q

Whta is a base

A

Substance which readily accepts H+ ions

31
Q

How to prepare a solution

A

Weigh mass of crystals
Dissolve in water
Transfer to 250cm volumetric flask
Make up to mark with more water so that bottom of meniscus is on the mark
Use balance with 2 or more d.p
Use dropping pipette when adding water up to the mark
Use stopper when inverting 250cm^3 volumetric flask to mix solution

32
Q

What is a procedure that obtain graph of total mass against time

A

Use flask, balance and stopwatch and record at time intervals between 10 and 50s

33
Q

How could a student obtain sample of magnesium phosphate and reacting magneisum with phosphoric acid

A

Filter to obtain solid precipitate

Dry solid to remove water

34
Q

How would you reducre uncertainty

A

Use balance with more decimal places
Use a larger mass

35
Q

How would you make sure all water of crystalisation is removed

A

Heat to constant mass

36
Q

What is the defenition of an ionic lattice

A

Repeating pattern of oppositely charged ions

37
Q

What is the defenition of a covalent bond

A

Shared pair of electrons

38
Q

What is meant by the term standard solution

A

A solution of a known concentration

39
Q

How do you reduce random error in a titration

A

Repeat titration until you achieve concordant results within 0.1cm^3 of eachother

Calculate a mean titre from your achieved concordant results

Chemistry (4 decks)

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