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Physchem > Handbook 1 > Flashcards

Handbook 1 Flashcards

1
Q

What is the maximum number of electrons which can occupy a

i) 2p sublevel
ii) 2 p orbital

A

i) 6

ii) 3

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2
Q

Name the group on the periodic table whose elements are non-metallic and have a valency of 1

A

Group VII - Halogens

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3
Q

Define the term valency

A

Number of electrons that can be gained, lost or shared

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4
Q

What colour do Lithium salts give a Bunsen burner flame

A

Crimson/red

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5
Q

What colour do copper salts give a Bunsen Burner flame

A

Blue-green

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6
Q

Name the element that emits a yellow light during a flame test

A

Sodium

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7
Q

What do E2 and f represent in the equation E2-E1=hf

A

E2- Higher energy level

f- frequency of light

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8
Q

Distinguish between the terms ground and excited state

A

Ground state- Lowest available energy level

Excited-state- Higher available energy level

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9
Q

Distinguish between the terms atomic number and mass number

A

Atomic number- Number of protons

Mass number- Number of protons and neutrons

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10
Q

What does Aufbau’s principle state

A

When building up the electron configuration for an atom in its ground state the electrons occupy the lowest available energy level

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11
Q

List two limitations of Bohr’s theory

A

Electrons move in a wave motion

Heinsberg’s uncertainty principle

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12
Q

Distinguish between an atom and a compound

A

Atom is the smallest particle that has properties of an element
A compound is two or more elements that are chemically combined

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13
Q

What are isotopes

A

Atoms of the same element with the same atomic number and different atomic mass

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14
Q

What is an atomic orbital

A

A region of space where electrons are most likely to be found

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15
Q

Outline the procedure of flame test

A
  • Soak a wooden splint in water
  • Dip it in salt
  • Hold in the blue part of the Bunsen flame
  • Observe colour
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16
Q

What colour would Pottasium be in the flame test

A

Lilac

17
Q

What colour did Lithium salts give to a Bunsen burner flame

A

Crimson

18
Q

Explain why the second ionisation energy of an element is always higher than its first ionisation energy

A

Second electron is removed from a positive ion

19
Q

Define relative atomic mass

A

Mass of an atom compared to1/12th the mass of carbon 12- isotope

20
Q

Name two molecular crystals

A

Dry ice

Iodine

21
Q

2 Chemical properties associated with transition metals

A
  • Variable valency

- Acts as a catalyst

22
Q

Define Heinsberg’s uncertainty principle

A

It is impossible to measure both the velocity and the position of an electron at the same time

23
Q

Define the first ionisation energy of an element

A

The minimum energy required to remove the most loosely bound electron from a neutral gaseous atom in its ground state

24
Q

The general rule for first ionisation energy across a periodic table

A
  • IE value increases
  • Atomic radius is decreasing
  • Effective nuclear charge is increasing
  • Screening effect remains the same
25
Q

explain why fi value of beryllium is larger than that of boron

A

Be- has a higher value as it has a full s-sublevel
(2s2) and is stable
B- Has a lower value as the p-sublevel is (2p) and is not stable

26
Q

Define Ionic bond

A

The force of attraction between oppositely charged ions due to the transfer of electrons

27
Q

Describe the crystal structure of sodium chloride

A

Crystal lattice
Sodium ions are surrounded by 6 chloride ions
Each chloride ion is surrounded by 6 sodium ions

28
Q

Give two general properties of ionic compounds

A
  • Conduct electricity when dissolved in water
  • Form solid crystal lattice structures
  • Compound of ions
  • Have high melting or boiling points
29
Q

Define intermolecular forces

A

Force of attraction between molecules

30
Q

Name the type of intramolecular bonding in

i) Ammonia gas
ii) Water
iii) Methane gas

A

i) Hydrogen Bonding
ii) Hydrogen bonding
iii) Van der waals

31
Q

Explain in terms of intermolecular forces why NH3 is very soluble in water

A
  • NH3 is a polar molecule
  • H2O is a polar molecule
  • Positive side of the H20 attracts the negative side of the NH3 molecule
  • The negative side of the H20 attracts the positive side of the NH3
    “Like dissolves like”
32
Q

Describe the bonding in Cl2

A

Pure covalent bond

33
Q

Define electronegativity

A

The measure of the force of attraction an atom has for a shared pair of electrons in a covalent bond

34
Q

Why do electronegativity values increase across the third period of the periodic table

A
  • Atomic radius decreases
  • Electric nuclear change increases
  • Screening effect remains the same

Physchem (4 decks)

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