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GAMSAT general chemistry > Ionisation energy > Flashcards

Ionisation energy Flashcards

1
Q

define electronegativity

A

how much an atom pulls on electroncs in a bond

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2
Q

metallic character define

A

how easily an atom gives up an electron in a bond

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3
Q

how does the metallic character change across the table?

A

decreases across the table because more protons in nucleus attracting electrons and increases down the table

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4
Q

how does the electronegativity change across the table and down?

A

increases across table and decreases down the table

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5
Q

how does the reactivity change across table table?

A

increases up and right and down and left

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6
Q

ionisation energy -trend left to right?

  • increase
  • decrease
A

increases with increasing atomic number

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7
Q

Ionisation energy from top to bottom?

A

Decreases as atomic size increases

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8
Q

What does Electronegativity depend on?

A
  1. The nuclear charge
  2. The radius
  3. The shielding of the nuclear charge by electrons in inner shells
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9
Q

What are the most electronegative atoms?

  • Flourine,
  • Nitrogen,
  • carbon
  • Na
A

Flourine has the ‘most electron pulling power’

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10
Q

Which means ionisation energy?

  • energy needed to pull an electron away from the attraction of the nucleus
  • electron pulling power
A

energy needed to pull an electron away from the attraction of the nucleus

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11
Q

anion is …

a positively charge ion
a negatively charge ion

A

negative

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12
Q

a cation is

a ion with additional electrons
an ion with removed electrons

A

an ion with additional electrons

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13
Q

in NaCl - the Na is :

  • a cation
  • an anion
A

a cation

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14
Q

The sodium ion is positively charge because it has

  • lost a negative
  • gained a negative

electron.

A

lost a negative ion

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15
Q

The attractive energy can be expressed as follows:

E=(kq1q2/r)
E = k/r *q1q2
E=kq1q2/r2

A

E= kq1q2/r

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16
Q

What does the q’s stand for in the equation for attractive energy?

E=(kq1q2/r)

A

charges on each ion

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17
Q

which has a shorter bond length? NaF or KCl

A

they have the same charge profile but Na and F are smaller so their bond is shorter. As bond length appears in the denominator of coulombs law, a shorter bond leads to a greater bond energy.

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18
Q

Phosphate is written how?

PO2 ^3-
PO4 ^3-
PO ^-
PO2 ^2-
PO4 ^2-
A

PO4 ^3-

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19
Q

NH4+ is named ammonia or ammonium.

A

Ammonium

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20
Q 
Carbonate is written how?
CO4^2-
CO^-
CO2^3-
CO3^2-
A

CO3^2-

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21
Q

Nitrate is written how?
NO3^2-
NO3^-
NO2^2-

A

NO3^-

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22
Q

Calcium chloride is written how?

A

CaCl2

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23
Q

Iron Sulfate (III)

is written how?

A

Fe2(SO3)3

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24
Q

what is a nonmetal vs nonmetal most likely to be bond-wise?

A

covalent

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25
what is a metalloid and nonmetal most likely to be - covalent or ionic?
covalent
26
nonpolar bonds occur when atoms ____share pairs - equally - non-equally
equally
27
if the electronegativity difference is between___ and __ the bond is polar
0.4 and 1.7
28
when is the bond ionic - i.e at what range of electronegativity difference.
1.7 and above
29
what does the strength of any metallic bond depend on?
the charge of the ion ad the size of the ion.
30
calculate the number of moles of oxygen at STP present in a volume of 78.75L
One mole of gas occupies a volume of 22.4L. To get the number of moles you have to divide 78.75L/22.4L/mol. = 3.5 moles
31
a 1L volume of a gas is at a pressure of 20 atm. A valve allows the gas to flow into a 12l container, connecting the two containers. What is the final pressure of this gas?
1.54 atm boyles law is pv=PV
32
1 atm = ___mmHg = ___ torr
760 mmHg and 760 torr
33
1 atm = ___Pa
1.01x10^5Pa
34
What is Charles' Law ?
Like boyles but constant pressure. V=kT VT=vt
35
What is Gay-Lussac's law?
Gay-lussac's law is expressed as: PT=pt constant Volume (gunpowder!)
36
A 20 L cylinder contains 6 atm of gas at 27C. What would the pressure of the gas be if the gas was heated to 77C?
volume is constant hence Gay lussacs law! PT=pt 7atm
37
Find the volume of a gas a STP when 2.00 liters is collected at 745.0 mmHg and 25.0 degrees celcius.
V2=1.80L Remember to convert to kelvin when using temperature. (+273)
38
convert 25.0 degrees into K
298K
39
6.2 litres of an ideal gas is contained at 3.0atm and 37c. How many moles of this gas are present?
The ideal gas law is pV=nRT. There are 0.75 mol of the ideal gas present in the system.
40
what is the ideal gas law?
pV=nRT
41
what are some of the assumptions of the kinetic theory of gases? Molecules are in __,__ motion. Collisions are (plastic/elastic). Walls of the containers are ___
Molecules are in constant, random motion. Collisions are elastic. rigid.
42
A balloon contains 0.1 moles of oxygen and 0.4 moles of nitrogen. If the balloon is at standard temperature and pressure, what is the partial pressure of the nitrogen?
0.8atm
43
A 1litre flask contains 0.4 mol of helium and 1.2 moles of hydrogen gas. Find the mole fractions and partial pressures of both gases, if the total pressure of the mixture is 790 mmHg.
The total number of moles of gases present in the container is 0.4 +1.2 = 1.6 moles. 197. 5 mmHg 592. 5 rnHg
44
What is daltons law? relates partial pressure of gas x Total pressure of all gases Number of moles of gas number of moles of all gases
Px=Ptotal (nx/ntotal)
45
which is faster effusion or diffusion?
effusion because of negative pressure. and they dont have to move around particles.
46
name three intermolecular forces
hydrogen dipole-dipole london forces
47
which is stronger a hydrogen bond or a dipole dipole?
a hydrogen
48
what are h bond represented as
a ----
49
what are the only atoms electronegative enough to form h bonds
NOF
50
Two sulphur dioxide molecules - the sulphur atom is attracted to the oxygen atoms of the other molecule. What is this an example of?
a dipole-dipole
51
the interaction between two methyl groups is an example of what?
london force
52
the force between two nonpolar molecules and is the weakest of the intermolecular forces. The electrons of one molecule are attracted to the nucleus of the other molecule. this is an example of what kind of force dipole london hydrogen
london force
53
What is the sum of the attractive and repulsive electrical forces between atoms and molecules called?
van der waals
54
what are the four types of solids?
ionic metallic molecular network
55
a molecular solid is held together by ___forces
intermolecular
56
ICE is an example of what kind of solid? - ionic - network - metallic - molecular
Molecular
57
In a network solid, the atoms are held together by ___
covalent bonds
58
a crystal is what kind of solid? | ionic, molecular, metallic or network?
network
59
NaCl is an example of what kind of solid?
An ionic solid.
60
The conversion of a liquid to a gas is called
vaporisation
61
direct conversion of a solid to a gas
sublimation
62
gas converting into a solid is called what?
deposition
63
What is it called when heated particles trasnfer heat to another substance such as cooking something in boiling water? radiation convection conduction
convection
64
blood circulation in warm blooded mammals is an example of what kind of heat trasnfer?
convection
65
what is the vapour pressure at the critical temperature called?
critical pressure
66
The lattice energy is ...
THE process in which oppositely charged ions in the the gas phase combine to form an ionic lattice in the solid phase.
67
molarity units?
mol/L
68
Express the concentration of a solution of 1.2 grams of KCl in 250 ml of water.
0.0644 M
69
How do you calculate molality?
moles of solute/kilograms of solvent
70
A 4g sugar cube is dissolved in a 350ml teacup of 80c water. What is the molality of the sugar solution? Given: Density of water at 80C=0.975g/ml.
0.033M
71
What is normality?
a measure of concentration equal to the gram equivalent weight per litre of solution.
72
a 1 molar solution would be called a ___ normal solution because it can _____
a 2 normal solution because it can donate 2 protons for each H2SO4.
73
calculate the molar solubility of silver chloride
x= 1.34x10^-5
74
most compounds that contain nitrogen are ___electrolytes - strong - weak
weak
75
Strong electrolytes include HCL HF NH3 H20
HCL
76
Is glucose a weak, strong or non electrolyte solution?
nonelectrolyte

GAMSAT general chemistry (11 decks)

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