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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!!

You may prefer our related Brainscape-certified flashcards:
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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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