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CHM 101 > Gross Features Of Atomic Structure ; Periodic Table > Flashcards

Gross Features Of Atomic Structure ; Periodic Table Flashcards

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1
Q

Who first proposed the existence of an atom in the 5th century

A

Leucippus and Democritus

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2
Q

What did Leucippus and Democritus say about the atom

A

” that matter cannot be endless divided and a continued sub- division of matter ultimately yield an atom

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3
Q

When did John Dalton propose the atomic theory

A

1803-1808

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4
Q

John Dalton proposed that??

A

The atom is the smallest indivisible particle of an element

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5
Q

Postulates of Dalton’s theory

A

i) Matter is made up of small indivisible particle called atoms
ii) Atoms can neither be created nor destroyed
iii) Atoms of the same element are identical or alike in every aspect but different from atoms of other elements
iv) Atoms combine to form compounds and they do so in simple whole number ratio
v) All chemical changes occur as a result of combination or separation of atoms

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6
Q

Limitations of Dalton’s theory

A

1)Dalton’s atomic theory did not explain or make provision for the possibility of existence of isotopes ( i.e atoms of the same element which have different masses)
2) A possiblity where some atoms of elements can combine in non- integral ratios
3) A reaction that could lead to creation or destruction of atoms ( atoms are created in nuclear fusion and destroyed in nuclear fission

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7
Q

Modifications of Dalton’s atomic theory

A

1) Atoms are divisible, as it contains other small particles such as protons, neutrons and electrons ( atoms are no longer indivisible particles)
2) Atoms can be created and destroyed in nuclear reaction
3) Atoms of the same elements are not identical or alike in every aspect due to existence of isotopes
4) In some larger or macro organic molecules compounds like polymers, atoms combine in non-integral ratios

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8
Q

Describe the atomic structure as proposed by Neil bohr

A

An atom has imaginary lines orbiting the nucleus and the line or orbits(shells) are situated at various distance from the nucleus.

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9
Q

What’re shells/orbits

A

They are imaginary lines orbiting or surrounding the nucleus of an atom . The assigned shells are K,L,M,N,O

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10
Q

What is the nucleus

A

Nucleus is the atomic Central core which is positively charged and contains protons and neutrons and most of the atomic mass.

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11
Q

When was the electron discovered

A

1897

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12
Q

What is an electron

A

Electron is a very light, negatively charged particle that exist in the region around or outside the positively charged nucleus.

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13
Q

What is a proton

A

A proton is a nuclear particle having a positive charge equal to (+e) and a mass more than 18000 times that of electron.

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14
Q

What is a neutron particle

A

Neutron is a nuclear particle having a mass almost identical to that of the proton but has no electrical charge.

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15
Q

When was the nucleus discovered

A

1932

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16
Q

Sub atomic particles

A

Electron
Proton
Neutron

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17
Q

What are the masses of the electron, proton and neutron

A

Electron: 1/1840
Proton: 1
Neutron: 1

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18
Q

What are the charges of electron, proton and neutron

A

Electron: -1
Proton: +1
Neutron: 0

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19
Q

What is an atomic symbol

A

Atomic symbol which is a one or two or three lettered notation used to represent an atom corresponding to a particular element

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20
Q

What is mass number or nucleon

A

Is defined as the number of protons and neutrons in the nucleus of atom of an element
Mass number = Number of protons + number electrons

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21
Q

What is atomic number

A

It is defined as the number of protons in the nucleus of an atom of an element or the number of electrons of an element outside the nucleus

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22
Q

What is isotropy

A

The phenomenon or occurrence or existence of two or more atoms of an element having the same atomic number but different mass number

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23
Q

What is mass spectrometric analysis

A

It is a technique only used to determine the exact number of isotopes of a element, the masses of the isotopes, percentage and fractional abundance of each isotopes using an instrument called mass spectrometer

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24
Q

What is fraction abundance

A

Fraction abundance of an isotope is the fraction of the total number of atoms that is composed of a particular isotope

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25
Q

What is percentage abundance

A

Percentage abundance of an isotope is the fraction of the total number of atoms that a particular isotope is composed of, expressed in percentage.

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26
Q

What is relative atomic mass

A

The relative atomic mass is defined as the mass of an atom of an element compared to 1/12 the mass of an atom of carbon - 12 isotope.

27
Q

What was the first metal to be discovered?

A

Sodium and potassium which were isolated by Humphry davis

28
Q

In what year did Dmitri Mendeleev create the periodic table

A

1869

29
Q

Dmitri Mendeleev an the German chemist ………… working independently made similar results

A

J.L other meyer

30
Q

Dmitri Mendeleev published that??

A

” when elements are arranged in order of Thier increasing atomic weight or masses their properties reoccur at certain intervals or are periodic in nature”

31
Q

Mendeleev postulates on periodic table

A

1) Chemical properties of elements are periodic function of Thier atomic masses or weight

32
Q

Definition of periodic table

A

A periodic table is a table arrangement of elements in rows and columns highlighting or showing the regular repetition of properties of elements.

33
Q

Differences between Mendeleev table and modern table

A

1)In Mendeleev’s table elements were arranged in order of Thier increasing atomic weight or masses.
Elements in the modern table are arranged in order of Thier increasing atomic number or protons.
2) in Mendeleev’s table gaps were created for future elements to be discovered
In the modern table no gaps are left for future elements

34
Q

The periodic table has 8 vertical columns called??

A

Groups or families

35
Q

The periodic table has 7 horizontal rows called??

A

Periods

36
Q

What are groups??

A

Groups are all elements that have the same number of valence electrons ( electrons on outer most shell)

37
Q

What are periods

A

Periods are all elements that have the same number of electrons shells.

38
Q

What is the periodicity of elements

A

Periodicity is the variation of the properties of elements in a regular pattern both down the group and across the periods.

39
Q

Define atomic radius

A

Atomic radius is defined as half the distance between the nuclei of two atoms of the same elements that are covalently bonded in a molecule.

40
Q

Trends/variation atomic radius in the periodic table

A

Atomic radius or size or volume/ ionic radius or size of atoms of elements decreases across any period from left to right and increases down any group of elements in the periodic table from top to the bottom.

41
Q

Reason for the trends in atomic radius

A

Atomic size or radius decreases across any period of elements in the periodic table from left to right due to increase in effective nuclear charge and no increase in the screening effect of inner shell across a period of elements.how it’s increases down the groups of elements due to addition of a new shell and also due to the screening effect of inner electrons.

42
Q

Define Ionization Energy (IE)

A

It is the energy required by neutral atom in it’s ground State to lose one or more of it’s electron from it’s outer most shell.

43
Q

Trends of Ionization Energy in the periodic table

A

Ionization Energy or the value of Ionization Energy increases across the period of elements from left to right and it decreases down the group of elements from top to the bottom.

44
Q

Reasons for the trends in ionization energy (I.E)

A

Ionization Energy increases across the period of elements from left to right due to increasing effective nuclear charge, decreasing atomic radius and decreasing metallic property across the period. However, it decreased down the groups of elements from top to the bottom due to increasing atomic radius. Screening effect of inner electrons and increasing metallic property of elements down the groups

45
Q

Factors affecting the ionization energy of an atom of elements

A

1) Atomic radius, size of an atom of elements
2) Nuclear charge
3) The shield effect or screening effect of inner electrons
4) Electron configuration
5) The penetration effect

46
Q

What is Electron Affinity (EA)

A

Electron Affinity is the energy required by an isolated gaseous atom to gain or accept electrons to form a negatively charged ion.

47
Q

Trends of Electrons Affinity (EA)

A

Electron Affinity or the value of electron affinity increases across the period of elements from left to right and it decreases down the group of elements from top to the bottom.

48
Q

Reason for the trends in electron affinity

A

Electron Affinity increases across the period of elements from left to right due to increasing effective nuclear charge, decreasing atomic radius and decreasing metallic property across the period. However, it decreases down the group of elements from top to the bottom due to increasing atomic radius, screening effect of inner electrons and increasing metallic property of elements down the group.

49
Q

What is electronegativity

A

It is defined as the measure of ability of an atom of an element in a covalent molecule to attract the bonded pair of electrons to itself.

50
Q

Trends of electronegativity in the periodic table

A

Considering the elements in period 2 and group 7A; electronegativity value of elements increases across the period of elements from left to right and decreases down the group of elements from top to the bottom. Electronegativity values of elements are obtained using Linus Pauling’s formula and values are unit - less or has no unit because they are obtained as a scale as this.

51
Q

What are metallic and non - metallic properties

A

Generally the metallic property of elements increases down the group of elements from top to the bottom and decreases across the period from left to right.
Whereas the non - metallic property of element decreases down the group from top to the bottom and increase across the period from left to right.

52
Q

What are boiling and melting points

A

For representative metals ( i.e group 1A - 4A metals) Thier boiling and melting points decrease down the group from top to bottom because metallic property increases across the periods from left to right because decrease in metallic property.
However, for non - metals Thier boiling and melting points increase down the group from top to the bottom and decrease across the periods from left to right.

53
Q

Metals that exist as liquid at room temperature

A
  1. Mercury
  2. Francium
  3. Gallium
  4. Caesium
  5. Rubidium
54
Q

Conditions required to achieve Before substances mix together

A
  1. Miscibility: two liquids that mix completely together are said to be miscible.
  2. Intermolecular forces: the ability of two different compounds to interact with each other depends on the types of intermolecular attraction they have.
  3. Chemical composition: A mixture is physical combination of two or more substances in which the identities are retained and are mixed in the form of solutions, suspension and colloids
    4) No chemical bonding: in a mixture, there is no chemical bonding between the ingredients substances retains its own chemical properties and make up
55
Q

Solubility of a solute in a solvent depends on??

A

A balance between the natural tendency for the solute’s and solvent specie to mix and the tendency for a system to have the lowest energy possible

56
Q

Solubility of molecular substances

A

For molecular substances, or substances like one gas dissolving in another or one liquid the only factor of importance that accounts for Thier solubility is the natural tendency for the molecules to mix as a result of having similar or near equal intermolecular forces of attraction.

57
Q

Define hydration

A

Hydration is defined as the attraction of ions of water molecules

58
Q

Definition of hydrates

A

A hydrate is a compound that contains water molecules weakly bound in it crystals. Hydrated substances are often obtained by evaporation of an aqueous solution of the compound.

59
Q

Define hydrolysis

A

The hydrolysis of an ion is defined as the reaction of a ion with water to produce the conjugate acid and hydroxide ion or the conjugate base and hydrogen ion

60
Q

Solubility of ionic substance’s

A

Ionic substances differ markedly in Thier solubility in water. In most cases, these differences in solubility can be explained in terms of the different energies between the ions in the crystal and between ions in water( i.e energy of hydration and lattice energy)

61
Q

Lattice energy

A

Lattice energy depends on the charge on the ion ( as well as on the distance between the centers of neighboring positive and negative ions). The greater the magnitude of ion charge the greater lattice energy and for this reason substances with singly charged ions are comparatively soluble and those with multiple charged ions are less soluble.

62
Q

Important consideration in hydrolysis of ions

A

1) prediction of whether a salt solution is acidic, basic or neutral
2) calculation of the concentration of H+ and OH- ion the salt solution ( or equivalent)

63
Q

Prediction of whether a salt solution is acidic, basic or neutral

A
  1. A salt of a strong acid and strong base has no hydrolysable ions and so give a neutral aqueous solution e.g Nacl, Kcl, Licl.
  2. A salt of a strong base and a weak acid the anion of the salt is the conjugate of the weak acid and it hydrolyzes to give a basic solution e.g
    Na2CO3, K2CO3
  3. A salt of weak base and a strong acid, the cation of the salt is the conjugate of the weak base and it hydrolyzes to give an acid solution. MgCl2, NH4Cl
  4. A salt of a weak acid and a weak base, both ions hydrolyzes and whether the solution is acidic or basic depends on the relative acid - base strength of the two ions e.g NH4CHO2
64
Q

What is hydrolysis equilibrium

A

Hydrolysis equilibrium occurs only when an ion can form a molecule of a weak electrolytes in the reaction with water.

CHM 101 (5 decks)

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