Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

BI1014 > Atomic structure, chemical bonds, chemical reactions, redox chemistry, pH and spectroscopy > Flashcards

Atomic structure, chemical bonds, chemical reactions, redox chemistry, pH and spectroscopy Flashcards

(64 cards)

Start Studying
1
Q

how is matter characterised?

A

by mass, colour, smell, density and melting point

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

atomic structure

A

nucleus and shell
nucleus contains majority of mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

isotope

A

atoms of the same element with different mass numbers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what subshells are there and how many electrons do they hold?

A

s: 2
p: 6
d: 10
f: 14

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

what are orbitals?

A

probability of the presence of an electron

number of nodes is dependent on main shell n and define kind of subshell, number of subshells reflect possible spatial orientation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

how is the energy level of an electron characterised?

A

4 quantum numbers
size of orbitals
shape of orbitals
orientation of orbitals
and spin

max 2 electrons per orbital

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

describe on the periodic table the s, p, d and f block

A

groups 1 and 2 are s
transitions are d
far right p
then at the very bottom is f

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

describe the radioactive isotopes

A

stability of nucleus - ration if neutron to proton with total charge
heavy nuclei - increasing number of protons with increasing charge
light nuclei - ‘odd’ of neutron to proton ratio

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

types of radiation

A

heavy produces alpha decay and alpha radiation
light and heavy nuclei produces beta decay and beta radiation
excited nuclei and excess energy produce gamma radiation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

what is alpha beta and gamma radiation shielded by?

A

alpha: paper, clothing (helium nucleus)
beta: heavy clothing, lab coat and gloves (electron)
gamma: lead, thick concrete (electromagnetic radiation)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

how is radiation measured?

A

activity: becquerel Bq
used to be in Curie Ci

absorbed: Gray Gy
radiation absorbed dose rad

biological damage: Sievert 1 Gy x factor Sv
radiation equivalent in humans rem

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

artificial radioisotopes

A

the conversion of stable isotopes into radioactive using fast moving particles (transmutation)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

applications of radioactivity

A

carbon dating
radio-immuno assay
medical (visualisation and treatment)
energy generation (fission and fusion)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what configuration is the most stable?

A

noble gases because it uses the octet rule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what types of covalent bonds are there?

A

polar - they form dipoles
dative/ coordinate - filled and vacant orbital to allow shared electron pair

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

features of crystal lattice

A

electrostatic force
macroscopic structure
depends on charge of ions to define its class

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

do covalent bonds have a specific length?

A

yes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

what is the valence shell electron pair repulsion theory (VSEPR)?

A

count the number of binding electron pairs and free electron pairs (bonding and lone pairs)
total number of and achieving maximal distance between pairs determines shape

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

what is the rations, problem and solution behind the valence bind theory?

A

rational: atoms bond in covalent bonds by sharing electrons in the valence shell, electrons are in orbitals at the atom
a bond is characterised by overlap of these orbitals
problem: atomic orbitals don’t reflect actual direction of bonds
solution:
mathematical mixing of orbital functions of s and p orbitals resulting in mixed (hybrid) orbitals (all hybrid orbitals have the same shape)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

can double covalent bonds rotate?

A

no

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

what shape are triple bonds generally?

A

linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

describe London forces (Van der Waals)

A

temporary difference in distribution of binding electrons causing temporary and partial positive and negative charges
attraction dependent on contact area
weakest of the intermolecular forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

describe dipole-dipole interaction van der Waals

A

based on permanently polarised bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

describe hydrogen bonds

A

requires oxygen or nitrogen in organic molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
describe the structure of water
water less dense when solid (ice floats) water bodies freeze from top down essential for evolution of life high boiling point
26
what are states of matter described by?
pressure (Pa) volume (m3) temperature (K) amount (mol)
27
what is the law of thermodynamics?
matter has an energy content heat is equivalent to mechanical energy energy content can only be changed by heat exchange and work with environment energy cannot be created nor destroyed
28
what equation links to the law of thermodynamics?
dH = deltaQ + delta W Q = adding or removing heat W = work dH = CpdT + Vdp
29
ideal gas law equation
pV=nRT R= 8.31441 JK-1mol-1
30
how are enthalpy formations calculated?
change in reaction = change in products - change in reactants
31
what is Hess's law?
the enthalpies of a reaction is equal to the sum of the enthalpies of the reactions into which it may be divided the enthalpy of a reaction is independent of the route taken
32
what is entropy?
a measure of disorder the larger the entropy, the more disordered
33
what does entropy usually stay as?
0 or is positive
34
what is Gibb's free energy? when is it spontaneous and not?
G = H-TS if its exergonic - spontaneous so less than 0 if its endergonic - non-spontaneous and is more than 0
35
what equations are used to measure entropy?
phase transitions accessible electrochemical reactions chemical equilibria
36
reaction rate
rate = k [X] power of a k= concentration of X if k is less than 1 the reaction is slow if k is more than 1 the reaction is fast
37
rate constant
k = z e -Ea/RT you know -Ea/RT is to the power
38
how do you tell if something is under thermodynamic control or kinetic control?
thermodynamic - k is more than 1 so exergonic reaction will happen kinetic - k is less than 1 so exergonic reactions will only happen when Ea is provided
39
bronsted-lowry acid and bases
acid - proton donor base - proton acceptor acid-base reactions form an equilibrium, the equilibria is dynamic
40
mass action law
kfor/kback = k=[C][D]/[A][B] K is the equilibrium constant c and d are the product concentrations a and b are reactant concentrations
41
principle of LeChatelier
when a stress is imposed on an equilibrium, the reaction will shift to relieve the stress in either concentration, pressure or temperature
42
give an example of a weak acid and a weak base an then an example of a strong acid
wa = acetic acid wb = acetate ion sa = hydrochloric acid
43
salt
product of neutralisation of acid and base neutralised salt contains equivalent amount of acid and base pH of the salt solution is not always neutral
44
ampholytes
salts of weak acids and weak bases (ammonium acetate) hydrogen salts (di or triprotic acids) compounds with acid and base functional groups (AAs) pH independent of concentration pH= pKa1+pKa2/2 use that equation on titration curves too
45
buffers
solution of weak acid or base and its conjugate base or acid = salt solutions of ampholytes
46
pH = pKa +log[A-]/[HA]
shifted by value of pKa not suitable to calculate 100% acid or base
47
oxidation number in molecular compounds
the more electronegative element gets negative charge bonds between the same element do not count towards oxidation numbers sum of oxidation number equals 0 or ionic charge in case of polyatomic ions
48
name the exceptions for oxidation numbering
hydrogen is the most electronegative except hydrides (LiAlH4 where H-1) oxygen most electronegative except F2O oxygendifluoride O2+
49
electrochemical cell
anode - oxidation takes place, e flows out and is positively charged and attracts negatively charged ions cathode - reduction takes place, e flow in, is negatively charged and attracts positively charged ions
50
to calculate change in enthalpy
look at half reactions table rearrange with the more negative half reaction on top combined reactions rub anticlockwise reverse top half-reaction (negative becomes positive) add the potentials with a chage that is more than zero happens spontaneously - battery discharge application of voltage to reaction forces its reversal - battery charging
51
deltaG = z.F. deltaE z= number of electrons F= faraday constant = 96485.309C/mol
52
what's on the electromagnetic spectrum
radio microwave infrared ultraviolet gamma mobile radar visible x-ray
53
how is frequency calculated?
1/s
54
what is snells law
n1sin1=n2sin2 n= refractive index n= speed of light in vacuum/speed of light in medium (c/v)
55
what type of interference waves can you get?
constructive - crests and troughs align - field strengths add up for each point destructive - crests align with troughs - 180 degrees out of phase
56
beer's law
A = e. c. d e = molar absorptivity (L/mol/cm) c = concentration (mol/L) d = path length (cm)
57
what do waves show?
refraction, diffraction interference and polarisation
58
energy of electro-magnetci radiation is quantized by
E= hv absorption of electro-magnetic radiation in a stepwise increase of energy of specific movements of atoms and molecules: – Translation, rotation, vibration and electronic excitation – Energy required for excitation increases in order translation < rotation < vibration < electronic excitation
59
fluorescence and phosphorescence
wavelength gamma em of emitted radiation always longer than that of excitation gamma ex
60
emission intensity is proportional to...
concentration p = kc
61
applications of UV-vis spectroscopy
direct quantitative measurement of coloured substances and fluorescent substances tagging of targets with absorptive or fluorescent molecules histochemistry and imaging dynamic interaction
62
how are double bonds useful for UV-vis spec?
Double-bonds are essential for absorbance especially in visible area
63
what is mass spec based on?
manuipulating ions in the gas phase - molecules need to be ionized and vaporised. * Ion source creates ions and accelerates all with constant energy. Three main source: * Electron impact ionization (EI) * Electrospray ionization (ESI) * Matrix-assisted laser desorption ionization (MALDI)
64
what is fragmentation?
EI results in molecules breaking up = fragmentation * Fragmentation characteristic for chemical classes and can be predicted to a point.

BI1014 (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions