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Foundations in chemistry Flashcards

(71 cards)

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1
Q

What is an isotope?

A

atoms of the same element with same number of protons different number of neutrons

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2
Q

What is the structure of an atom?

A

nucleus made up of protons ans neutrons
electrons occupy shells

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3
Q

what is relative isotopic mass?

A

the mass of an isotope relative to 1/12th the mass of carbon-12

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4
Q

what is relative atomic mass?

A

the weighted mean mass of an atom relative to 1/12th the mass of an atom of carbon-12

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5
Q

what is amount of substance

A

the number of particles in a substance

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6
Q

what is Avogadro’s constant

A

6.02 x 10^23

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7
Q

what is molar mass

A

the mass per mole

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8
Q

what is empirical formula?

A

the simplest whole number ratio of atoms of each element in a compound

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9
Q

what is molecular formulat

A

the number and type of atoms of each element in a molecule

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10
Q

what does the term hydrated mean in terms of water of crystallisation?

A

a crystalline compound containing water molecules

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11
Q

what does anhydrous mean in terms of water of crystallisation

A

containing no water molecules

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12
Q

what does water of crystallisation mean

A

water molecules that are bonded into a crystalline structure of a compound

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13
Q

what is the formula for moles in terms of mass

A

moles = mass/ mr

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14
Q

what is the formula for moles in terms of gas volume

A

moles = vol / gas volume
at RTP moles = vol/ 24dm^3 or 24000cm^3

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15
Q

what is the formula ro moles in terms of conc

A

moles = concentration x volume (dm^3)

moles = (conc x vol in cm^3) / 1000

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16
Q

what is the ideal gas equation

A

pV= nRT
p= pressure (Pa)
V= volume (m^3)
n= moles
R= 8.31 J mol-1 K-1
T= temperature (K)

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17
Q

what is the formula for percentage yield

A

percentage yield= (actual yield/ theoretical yield) x 100

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18
Q

what is the formula for atom economy

A

(molar masses of desired products / molar masses of all products) x 100

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19
Q

what is a strong acid?

A

completely dissociates into a H+ ions when in an aqueous solution (water)

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20
Q

what is a weak acid?

A

partially dissociates into H+ when in an aqueous solution (water)

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21
Q

what is an alkali

A

a base that dissolves in water releasing hydroxides

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22
Q

what is neutralisation

A

H+ ions from an acid react with OH- ions from a base to form a salt and water

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23
Q

what are the products of the reaction of an acid with an alkali

A

acid + alkali = salt + water

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24
Q

the process of preparing a standard solution

A

-weigh out solid
-disolve solid in beaker using distilled water, stir with a glass rod
-rinse remaining solid from glass rod into beaker
-transfer solution to volumetric flask, use distilled water to rinse remaining solid into vf
-carefully fill flask with water to graduationline- add distilled water a drop at a time until the bottom of the meniscus is at the line
-slowly invert volumetric flask several times to mix the solution thoroughly

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25
what is the oxidation number for elements
always 0
26
how to work out oxidation numbers
sum of oxidation number= overall charge
27
what is a redox reaction in terms of electron transfer
reduction = gain of electrons oxidation = loss of electrons
28
what is a redox reaction in terms of changes in oxidation numbers
reduction= decrease in oxidation number oxidation= increase in oxidation number
29
what is the order of shells
s p d f
30
how many electrons fill first 4 shells
shell 1= 2 electrons (1s) shell 2= 8 electrons (2s + 2p) shell 3= 18 electrons (3s + 3p + 3d) shell 4= 32 electrons (4s + 4p + 4d+ 4f)
31
what is an orbital
a region around a nucleus that cah hold up to two electrons, with opposite spins
32
what is the shape of the s orbital
spherical
33
what is the shape of a p orbital
dumb-bell shape
34
how many orbitals are in the s sub shell and how many electrons can fill them
one s orbital one or 2 electrons in orbital
35
how many orbitals are in the p subshell and how many electrons make it up
3 orbitals total of 6 electrons- 2 in each orbital
36
how many orbitals and electrons make up the d sub shell
5 orbitals 10 electrons- 2 in each sub shell
37
what is the order of filling orbitals
1s 2s 2p 3s 3p 4s 3d 4p 4d 4f
38
what is the electrons in box model
electrons shown by arrows, since there is an opposite spin each arrow is facing a different direction
39
why does one electron (arrow) occupy each orbital before pairing
prevents repulsion between paired electrons until there is no further orbital available at the same energy level
40
what is ionic bonding
electrostatic attraction between positive and negative ions
41
what is the structure and properties of a giant ionic lattice
-each ion attracts oppositely charged ions in all directions -solid at room temperature there is insuffiient energy to overcome the strong electrostatic forces of attraction between oppositely charged ions -high temperatures needed to overcome the strong electrostatic attraction between ions so high melting and boiling pointd -ionic compounds dissolve in polar solvents (water) as the break down the latticr and surround each ion in solution -ionic compound does not conduct electricity in solid state as ions are in a fixed position so no mobile charge carriers
42
what is covalent bonding
the strong electrostatic attraction between a shared pair of electrons and the nuclei of bonded atoms an overlap of atomic orbitals
43
44
what is a dative covalent bond
a covalent bond in which the shared pair of electrons has been supplied by one of the bonding atoms only shared electron pair was originally a lone pair of electrons on one of the bonded atoms shown by an arrow (-->) to show which atom provides both electrons to the covalent bond
45
what is average bond enthalpy
a measurement of covalent bond strength - larger value = stronger covalent bond
46
what is the electron- repulsion theory
electron pairs repel each other so that they are as far apart as possible
47
bonding pairs vs lone pairs repulsion
lone pairs slightly closer to central atom, repel more strongly than a bonding pair
48
hoe much is the bonding angle reduced by for each lone pair
2.5 degrees
49
how to calculate lone pairs
total valence electrons for atoms (group number) - total bonding pairs
50
tetrahedral shape
**109.5** 4 bonding pairs 0 lone pairs
51
linear shape
**180** 2 bonding pairs 0 lone pairs
52
trigonal planar shape
**120** 3 bonding pairs 0 lone pairs
53
non linear shape
**104.5** 2 bonding pairs 2 lone pairs
54
trigonal pyramidal shape
**107** 3 bonding pairs 1 lone pair
55
trigonal bipramidal shape
**120, 90** 5 bonding pairs 0 lone pairs
56
octahedral shape
**90** 6 bonding pairs 0 lone pairs
57
what is electronegativity
the ability of an atom to attract the bonding electrons in a covalent bond
58
what is the trend of elecronegativity in the periodic table
increases across the period and up the groups
59
what is a non-polar bond
the bonded electron pair is shared equally between the bonded atoms (the bonded atoms have same or similar electronegativity)
60
what is a polar bond
the bonded electron pair is shared unequally between the bonded atoms ( have different electronegativity values)
61
what are the three different intermolecular forces
induced dipole-dipole interactions permanent dipole-dipole interactions hydrogen bonding
62
what are induced dipole-dipole interactions
result from interactions of electrons between molecules more electrons= larger the induced dipoles greater the induced dipole dipole interactions stronger the attractive forces between molecules
63
what are permanent dipole-dipole interactions.
- act between permanent dipoles in different polar molecules
64
what is hydrogen bonding?
a type of permanent dipole-dipole interaction found between an electronegative atom with a lone pair of electrons (oxygen, nitrogen, fluorine) and a hydrogen atom attached to an electronegative atom (H-O, H-N, H-F)
65
where does a hydrogen bond form?
-between a lone pair of electrons on an electronegative atom in one molecule and a hydrogen atom in a different molecule
66
what is the strongest type of intermolecular force?
hydrogen bonds
67
what are hydrogen bonds shown by?
a **dashed line** --------
68
what are the anomalous properties of water?
- solid ice is less dense than liquid water -water has a relatively high melting point and boiling point -relatively high surface tension and viscosity
69
why is solid ice less dense than liquid water?
- hydrogen bonds hold water molecules apart in an open lattice structure - water molecules in ice are further apart than in water - solid ice is less dense than liquid water and floats
70
why does water have a relatively high melting and boiling point?
-large amount of energy needed to break the hydrogen bonds in water
71
what is the structure and properties of a simple molecular substance?
structure: -molecules are held in place by weak intermolecular forces -atoms within each molecule are bonded together strongly by covalent bonds properties: -weak intermolecular forces can be broken by small amounts of energy so low melting/ boiling points -non-polar simple molecular substances tend to be soluble in non-polar solvents -simple molecular substances tend to be insoluble in polar solvents -do not conduct electricity as no mobile charged carriers

Chemistry (5 decks)

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