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sem - 1 Flashcards

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1
Q

Who created the 1st periodic table & when?

A
  • Dmitri Mendeleev published the 1st periodic table in 1869
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2
Q

How was Dmitri Mendeleev’s periodic table organized?

A
  • organized in order of increasing atomic mass
  • the new version of the P.T arranges the elements based on increasing atomic number
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3
Q

What similarities do elements within a group show?

A
  • similar chemical properties & reactivity b/c they have the same number of valence electrons
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4
Q

Differentiate between metals & nonmetals.

A
  • metals are great conductors of heat & electricity where as nonmetals are poor conductors of the two
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5
Q

Which groups on the periodic table have the most reactive elements?

A
  • group 1 = alkali metals
  • group 7 (VII) = halogens
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6
Q

What are valence electrons and what do they do?

A
  • they are the electrons on the outermost shell of an atom
  • they participate in the sharing or exchanging of electrons between other atoms which is responsible for chemical rxns
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7
Q

What are the 3 factors that the attraction between the positive nucleus and valence electrons depend on?

A

1- number of protons in the nucleus
2- distance from the nucleus
3- shielding effect of other e- closer to the nucleus

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8
Q

What is the effective nuclear charge (Zeff)?

A
  • it is the nuclear charge of an electron when both the actual nuclear charge ‘Z’ (the atomic # of the element) and the repulsive effects (shielding e-) are taken into account.

Zeff = Z (the atomic number/number of protons of the element) - S (the total number of shielding e-)

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9
Q

In the Zeff = Z - S (or sigma sign) formula, the sigma is called what?

A
  • it is called the shielding constant & it is greater than 0 but less than ‘Z’
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10
Q

Zeff (effective nuclear charge) increases which ways on the periodic table?

A
  • increases moving left to right
  • increases moving down the periodic table (per slaters rule)
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11
Q

What is slaters rule?

A
  • his rule calculates sigma (S) by accounting for the effective shielding of e- in each orbital shell
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12
Q

Define atomic radius.

A
  • it is the distance between the nuclei of two combined/adjacent atoms
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13
Q

How does the atomic radius vary going left to right across a period? Why?

A
  • the atomic radius decreases
  • because there is an increase in atomic # (Z) so there is an increase in the number of protons in the nucleus. this means there is an added e- to the same energy level and that causes Zeff to increase. There will be a bigger attraction and so the atomic radius decreases. (Think of class increasing the number of students analogy)
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14
Q

How does the atomic radius vary going down a group? Why?

A
  • atomic radius increases
  • because more protons means more e-. The e- enter another energy level so there is now a greater distance between the nucleus and outermost shell.
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15
Q

What is ionic radius?

A
  • it is the radius of a cation (when an atom has more protons than e-) or an anion (when an atom has more e- than protons)
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16
Q

How does the ionic radius change when we form an anion (X-)?

A
  • ionic radius increases
  • Cl = 17+ protons & 17- electrons
  • Cl- = 17+ protons & 18- electrons
  • the additional electrons cause a greater repulsion amongst the e- so size increases.
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17
Q

How does the ionic radius change when we form an cation (X+)

A
  • it decreases
  • Na = 11+ protons & 11- electrons
  • Na+ = 11+ protons & 10- electrons
  • we get rid of an electron so now there are less electrons which means there is less repulsion amongst the electrons so size decreases.
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18
Q

Define what isoelectronic is.

A
  • it is when 2 elements have the same electron configuration (or same # of electrons)
  • ex: Na+ = 11+ protons & 10- electrons
    Mg +2 = 12+ protons & 10- electrons

both have electron configuration of

1s^2 , 2s^2 , 2p^6

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19
Q

Is the ionic radius of a dispositive ion greater or less than the radius of a unipositive ion? Explain.

A
  • ionic radius is less than the unipositive one
  • This is b/c the dipositive ion has a bigger nucleur charge, therefore causing a bigger attraction so the size of the radius decreases.
  • example:
    Na+ = 11+ protons , 10- electrons
    Mg 2+ = 12+ protons , 10 - electrons
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20
Q

Is the ionic radius of a dinegetive ion larger or smaller than the radius of a uninegetive ion? Explain.

A
  • dinegetive ion has radius that is larger than the radius of a uninegetive ion
  • b/c there are 2 more electrons than protons so attraction is weaker (so bigger size) whereas the uninegetive ion only has 1 more electron than proton so attraction is still strong.
  • example:
    O -2 = 8+ protons , 10 e-
    F -1 = 9+ protons, 10 e-
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21
Q

We know that ions move through tiny channels in cell membranes. However, some channels allow ____ through but not larger than ____ ?

A
  • allow Na+ through
  • but not larger than K+
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22
Q

Define ionization energy (IE)

A
  • it is the minimum energy required to remove the most loosely bound electron from a gaseous atom in its ground state.
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23
Q

Define and give examples of 1st VS 2nd VS 3rd ionization energies.

A
  • First ionization energy (IE 1) is the removal of the first most likely bound e- from 1 mol of the gaseous atom to produce 1 mol of gaseous atom with a +1 charge
  • Second ionization energy (IE 2) is the removal of the most likely bound e- from 1 mol of the gaseous ion with the +1 charge to produce a mol of gaseous ion with a +2 charge
  • Third ionization energy (IE 3) is the removal of the third most likely bound election
  • Examples:(IE 1) = Mg (g) —> Mg+ (g) + e-
    (IE 2) = Mg+ (g) —> Mg +2 (g) + e-
    (IE 3) = Mg +2 (g) —> Mg +3 (g) + e-
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24
Q

How does ionization energy vary going across a period Vs down a group?

A
  • increase going across a period b/c number of protons (aka nuclear charge) increases so bigger attraction to the electrons. bigger attraction means bigger ionization energy b/c more energy is needed to pull the e-
  • decreases going down a group b/c there is a greater distance between the nucleus & outermost shell/electron. distance weakens attraction between the nucleus and outermost electron so less energy is required to steal that loose electron.
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25
Q

What are the exceptions to the trend in ionization energy? Why?

A
  • [ Be and B ]

Be comes before B so it’s ionization energy should be lower but it’s actually higher.

This is because ‘Be’ Electron configuration is 1s^2 , 2s^2

whereas

‘B’ Electron configuration is 1s^2 , 2s^2 , 2p^1

The electrons in the ‘p’ orbital is further from the nucleus than electrons in the ‘s’ orbitals so they require less energy to removed

  • [ N and O ]

N comes before O so it’s ionization energy should be lower but it’s actually higher.

‘N’ has an electron configuration of 1s^2 , 2s^2 , 2p^3

whereas

‘O’ electron configuration is 1s^2 , 2s^2 , 2p^4

In oxygen, the electron is removed form a doubly occupied p orbital. In that doubly occupied orbital, the 2 electrons are repelling each other and so less energy is required to remove the e- than an e- in a half-filled orbital

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26
Q

Which group had the highest and lowest ionization energies?

A
  • Alkali Metals (group 1) - lowest ionization energy
  • Nobel Gases (group 8) - highest ionization energy
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27
Q

Define electron affinity.

A
  • is the negative change in energy that occurs when a neutral atom in gaseous state gains an e- , releasing energy in the process. This makes the atom now an anion
  • the likelihood of a neutral atom to gain an e-
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28
Q

What is the difference between high Vs low electron affinity?

A
  • high EA = atom more easily accepts electron
  • low EA = atom less easily accepts electron
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29
Q

F (g) + e- —> F- (g)

Energy = -328 kJ mol^-1

So electron affinity is + 328 kJ mol^-1

Explain this.

A
  • fluorine accepts an electron and becomes F- all the while releasing energy.
  • Since releasing energy is an exothermic process, the change in energy has a negative sign which means that the electron affinity is positive.
  • The more positive or the more higher the Electron affinity of an atom indicates that the atom can more easily accept an electron
30
Q

Define electronegativity.

A
  • it’s the ability of an atom to attract electrons towards itself while in a chemical bond.
  • nonmetals tend to be electronegative (get electrons) while metals tend to be electro positive (give away electrons)
31
Q

What is the most electronegative element? Why?

A
  • Fluroine.
  • Because it has a high electron affinity (tends to pick up e- easily), high ionization energy (does not lose electrons easily), and it has a high nuclear charge with little shielding
32
Q

Explain the movement of dipole in H-F.

A
  • F is more electronegative than H (can attract e- toward itself more strongly) so the movement of the e- goes towards F————>
    H - F
33
Q

Describe the electronegativity trend on the periodic table.

A
  • increases across a period (left to right)
  • decreases going down a group
34
Q

What is a molecule?

A
  • two or more atoms held together via chemical forces/bonds
  • can contain atoms of the same element or atoms of two or more elements
35
Q

What is a diatomic molecule?

A
  • a molecule that contains only 2 atoms
  • ex: O2, H2, B2, Br2, HCl, CO
36
Q

What is a polyatomic molecule?

A
  • a molecule that contains more than 2 atoms
  • ex: H2O, O3, NH3, CH4
37
Q

What is a molecular formula?

A
  • it shows the exact number of atoms of each element in a molecule
  • ex: Glucose —> C6H12O6
    C = 6 atoms
    H = 12 atoms
    O = 6 atoms
38
Q

What is atomic mass?

A
  • the mass of the atom in atomic mass units (amu)
39
Q

1 amu (atomic mass unit) is defined as what?

A
  • a mass equal to 1/12 the mass of one carbon-12 atom
40
Q

Define average atomic mass.

A
  • the average mass of all the naturally occurring isotopes of the element.
  • mass x abundance %
41
Q

Define molecular mass/weight.

A
  • it is the sum of the atomic masses (in amu) in a molecule
  • ex: SO2

1S = 32.07 amu
2O = 2 x 16 amu
—————————
SO2 = 64.07 amu

42
Q

For any molecule

Molecular mass (amu) = molar mass (grams/mol)

A

1 molecule of SO2 = 64.07 amu
1 mol of SO2 = 64.07 g SO2

43
Q

What is a chemical reaction?

A
  • process in which a substance is changed into 1 or more new substances
44
Q

What is Avogadro’s number?

A

6.022 x 10^23

45
Q

1 mole of atoms = how many atoms?
1 mole of molecules = how many molecules?

A

• 6.022 x10^23 atoms
• 6.022 x10^23 molecules

46
Q

What is molar mass?

A
  • mass in grams of 1 mole of molecules or 1 mole of atoms
  • unit for molar mass is g/mol
47
Q

1 mole of atoms contains 6.022 x 10^23 atoms and has what kind of mass?

A
  • atomic mass
48
Q

1 mole of molecules contains 6.022 x 10^23 molecules and has what kind of mass?

A
  • molecular mass
49
Q

Difference between solute vs solvent?

A
  • solute = substance being dissolved
  • solvent = substance doing the dissolving
50
Q

What is a solution?

A
  • homogeneous mixtures of 2 or more substances that can be formed in any state of matter

Example:

Solute (NaCl) + Solvent (H2O) = Saline solution

51
Q

The human body is made up of what percentage of water?

A
  • 60%
52
Q

The body is comprised of how many L of

a) water
b) blood plasma
c) intracellular fluid
d) extracellular fluid

A

a) 40 L
b) 3 L
c) 25 L
d) 12 L

53
Q

What is a solution concentration?

A
  • the concentration of a solution is the amount of solute present in a given amount of solvent or solution
54
Q

Explain the difference between dilute solution and concentrated solution.

A
  • dilute solution = contains relatively little solute in a large quantity of solution
  • concentrated solution = contains relatively large amounts of solute in a given quantity of solution
55
Q

What are the two quantitative ways to measure the concentration of a solution?

A
  • using concentration percentage
    • used in clinical reports, medicines, IV drips, etc.
  • molar concentration (molarity)
56
Q

Units of measure of water:

a) 1 ml = ? grams
b) density = ?

A

a) 1 gram
b) d = m/v

57
Q

What is the Intravenous Drip (IV drip)?

A
  • it is the giving of substances directly into a vein
58
Q

Why would one need intravenous drip therapy?

A
  • when they can’t swallow safely due to being under a coma or anaesthesia
  • when they require medication which are destroyed by their gastric juices or are poorly absorbed by the gastrointestinal tract
  • when they must rapidly increase the concentration of medication (morphine) or electrolyte
  • when they can’t drink enough to keep up w/ the loss of fluids (major burns. Severe diarrhoea, haemorrhage, etc)
59
Q

Is the I.V drip hypertonic, isotonic, or hypotonic w/ the blood plasma?

Explain your choice

A
  • it is isotonic w/ the blood plasma
  • example: severe hydration.

If you inject water directly, RBC will swell and burst (Haemolysis). This would be hypotonic.

In the I.V drip, there is 5% w/v glucose. This is nearly isotonic w/ blood plasma. As the glucose is metabolized, the water remains to rehydrate the body

60
Q

How can milligram percent (quantitative method of finding concentration %) be helpful?

A
  • blood urea nitrogen levels (BUN) level is measure in milligram %
  • BUN is used for newborn babies to check that their kidneys are working properly. Urea nitrogen is a waste product that the kidneys remove from the blood. Higher than normal BUN levels indicate that your kidneys aren’t working well. A BUN test can help uncover the issue early on so that treatment can be more effective
61
Q

What is the normal bun level?

A

7 - 21 mg urea / 100 mL blood
= 7 - 21 mg%

62
Q

What is the name/condition that refers to an ‘elevated bun level’?

A
  • azoremia
63
Q

What can azotemia (elevated BUN level) be caused by?

A
  • impaired renal function
  • dehydration (lack of fluid volume to excrete waste products)
  • excessive protein intake or protein catabolism
64
Q

What is the blood urea level of an infant suffering dehydration?

A
  • 32 mg%

(So 32 mg of urea per 100 mL of blood or 0.032 g of urea in 100 mL of blood = 0.032% w/v)

65
Q

What is ppm (parts per million) method of finding concentration of solution used for? Give an example

A
  • used to describe extremely dilute solutions
  • for ex: the concentration of toxic metals present in drinking water. some cpds are toxic to humans at 1 ppm
66
Q

What are redox reactions?

A
  • rxns that produce energy at the molecular level of life
67
Q

What are the 3 major purposes energy is required for?

A
  • muscle contraction & other cellular movements
  • active transport of molecules & ions
  • synthesis of macromolecules & other bio molecules from simple precursors
68
Q

Why cycle is the fundamental way of energy exchange in biological systems? Hint: it is the oxidation of food

A

ATP - ADP cycle

69
Q

When does oxidation occur?

A
  • when a molecule loses electrons, loses hydrogens, or gains oxygen
70
Q

What happens if a molecule undergoes oxidation?

A
  • it has been oxidized and said to be the reducing agent
71
Q

When does a reduction occur?

A
  • when a molecule does any of the following:
    • gains e-
    • gains hydrogens
    • loses oxygen
72
Q

What happens when a molecule undergoes a reduction?

A
  • it has been reduced & is said to be the oxidizing agent

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