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AS Level Chemistry > AS Physical Chemistry > Flashcards

AS Physical Chemistry Flashcards

Hey Yall! This deck aims to help you master the AS Physical Chemistry topics. I didn't separate them as others tend to do, and my purpose for doing so is for you to have a quick revise before any tests or exams you have, be it in the LRT or in the car on the way to school. Good Luck!!

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1
Q

Do you enjoy studying Chemistry?

A

I hope you do! Lets get started! :)

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2
Q

Define Atomic Number

A

The number of protons in the nucleus of an atom

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3
Q

Define Mass Number

A

The number of Protons + Neutrons in the nucleus of an atom

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4
Q

Define isotopes

A

Atoms of the same element with different mass numbers

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5
Q

Define an Ion

A

Charged particles formed by the loss or gain of electrons.

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6
Q

Define First Ionization Energy

A

The energy needed to remove 1 mole of electrons from 1 mole of atoms of an element in the gaseous state to form 1 mole of gaseous +1 ions.

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7
Q

Define Atomic Orbitals

A

Regions of space that can be occupied by a maximum of 2 electrons.

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8
Q

Define Atomic Radius

A

One-half the distance between 2 nuclei

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9
Q

How does Size of Nuclear Charge effect Ionization Energy?

A
  • When proton no. increases, IE increases
    • Larger nuclear charge causes greater
      attraction between nucleus and outer
      electrons
    • More energy is needed to overcome the
      attractive forces to remove out er electron.
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10
Q

How does the distance of outer electrons from the nucleus effect Ionization Energy?

A
  • When distance between nucleus and outer electrons increases, IE increases
    • Attractive forces btwn electrons in the outer
      shell and nucleus weaken as distance
      increases.
    • Less energy is needed to overcome the
      attractive forces to remove outer electron.
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11
Q

How does Shelding Effect effect Ionization Energy?

A
  • When no. of full electron shells between outer electrons and nucleus increases, IE decreases.
    • Sheilding: repulsion from electrons in inner
      shells reduce the attractive forces btwn the
      nucleus and outer electrons.
    • Less energy is needed to overcome the
      attractive forces to remove outer electron.
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12
Q

How does Spin-pair repulsion effect Ionization Energy?

A
  • Spin-pair repulsion between electrons in the same orbital makes it easier to remove an electron, IE decreases.
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13
Q

General trend of Ionization energy across Period 3

A

Increases

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14
Q

Why is the IE of Mg higher than that of Al?

A
  • Outermost electron in Al is in the higher 3p
    subshell, whereas outermost electron in Mg is
    in the 3s subshell.
  • Outermost electron in Al experiences more
    shielding.
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15
Q

Why is the IE of P higher than that of S?

A
  • A pair of electrons occupy one 3p orbital in one atom of S
  • Spin-pair repulsion causes removal of 1st electron to be easier.
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16
Q

Define Relative Atomic Mass

A

The weighted average of atoms of an element compared to the unified atomic mass unit.

17
Q

Define Relative Isotopic Mass

A

The mass of an atom of an isotope compared to the value of the unified atomic mass unit.

18
Q

State Avogardo’s Law

A

Equal volumes of all gases contain equal number of molecules provided they are at the same temperature and pressure

19
Q

VSEPR Theory

A
  • Deduces the shapes of molecules.
20
Q

Q. State the bond angles of the following geometrical shapes
a. Linear (one sided)
b. Linear (double sided)
c. Trigonal Planar
d. Tetrahedral
e. Trigonal Bipyramidal
f. Octahedral

A

a. 180
b. 180
c. 120
d. 109.5
e. 90,120
f. 90

21
Q

Q. Give an example of each of the following geometrical shapes:
a. Linear (double sided)
b. Trigonal Planar
c. Tetrahedral
d. Trigonal Bipyramidal
e. Bent/non-linear.
f. See-saw

A

a. CO2
b. BF3
c. CH4
d. NH3
e. H2O
f. SeF4

22
Q

Define Bond Energy

A

The energy required to break one mole of a bond in a molecule in the gaseous state.

23
Q

Define Electronegativity

A

The power of an atom to attract the bonding pair of electrons to itself

24
Q

Define Bond Polarity

A

The partial separation of charge when 2 different atoms are joined by a covalent bond, resulting in an unequal sharing for the bonding pair of electrons.

25
Q

Describe a Polar Covalent Bond

A
  • where the electron distribution is permanently asymmetric / unequal
  • there is a separation of charge btwn atoms
  • partial +ve and partial -ve
26
Q
A

AS Level Chemistry (3 decks)

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