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Chemistry Unit 1 How To Pass Book > Atomic Orbitaks, Electronic Configuration And Perioc Table > Flashcards

Atomic Orbitaks, Electronic Configuration And Perioc Table Flashcards

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1
Q

How to electrons behave in an atom

A

Behave as standing waves in an atom. These are aves that vibrate in time but do not move in space

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2
Q

Describe orbitals

A

Different sizes and shapes of standing wave possible around the nucleus. Orbitals an hold a maximum of two electrons

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3
Q

How many orbitals are ther

A

4-s,p,d and f

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4
Q

What are atomic orbitals

A

Regions where there is a high probability of finding the electrons

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5
Q

What are the 4 quantum numbers

A

Principle quantum number (n). Angular momentum quantum number (Ms). Magnetic quantum number (Ml). Spin magnetic quantum number (Ms)

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6
Q

What does an orbital hold

A

A maximum of two electrons with opposite spin

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7
Q

What are the orbitals in an isolated atom

A

Each shell is said to be degenerate

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8
Q

What are atomic orbitals

A

The regions where there is a high probability of finding an electron

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9
Q

Describe s orbitals

A

All s orbitals a spherical in shape. Their diameter increases as the shell number increases. The only orbital present in the first shell

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10
Q

Describe p orbitals

A

Dumbbell shape. Only occur from the second shell onwards. These orbitals have equal energy and are said to be degenerate. Second shell has 1s and 3p orbitals

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11
Q

Describe the 3rd shell

A

Can hold a maximum of 18 electrons. Two electrons are held in the s orbital and another six are held in the three p orbitals meaning 10 electrons are held in the d orbitals therefore 5 d orbitals in the third shell

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12
Q

What shows evidence of atomic orbitals

A

Emission spectra of elements with more tHan on electron

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13
Q

What’s quanta

A

Certain fixed amounts of energy posed by an electron

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14
Q

Whats the quantum theory

A

States that the energy if an electron can be defined in terms of for quantum numbers

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15
Q

Whats principles quantum number

A

Each shell is described by a number known as this. This number indicates the electrons main energy level and related to orbital size. First shell n=1 and so on

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16
Q

The higher the value fo the principle quantum number the what

A

The higher the potential energy associated with the shell and the further from the nucleus the electron is likely to be found

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17
Q

What’s angular momentum quantum number

A

The shape of the sub shell is given by this. If value l=0 the electron is found in the s orbital, if l=1 electron found in the p orbital and so on

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18
Q

Whats magnetic quantum number

A

The orientation in space of the electron in different degenerate orbitals values between -1 and +1

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19
Q

Whats spin magnetic quantum number

A

Indicates the direction in which the electron is spinning its either clockwise or anticlockwise with values +1/2 and -1/2 electrons occupying the same orbital must have opposite spins

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20
Q

What are the orbitals within each subshell of an isolated atom

A

They are degenerate

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21
Q

What does the Pauli exclusion state

A

That no two electrons in one atom can have the same set of four quantum numbers. In other words no orbital can hold more than two electrons and they must have oppsite spins

22
Q

Whats the aufbau principle

A

States that orbitals are filled in order of increasing energy

23
Q

What is hunds rule

A

States that when degenerate orbitals are available/ electrons fill singly keeping their spins parallel before spin pairing starts

24
Q

Whats the filling order for sub shells

A

1s,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p,7s etc

25
Q

What is isoelectronic

A

Particles which have the same electronic configuration

26
Q

Learn copper and chromium electro ionic configuration of by heart as they don’t follow the rule

A
27
Q

Whats ground state

A

When electrons are in their lowest possible energy levels the atom is said to be in the ground state

28
Q

Learn how to right electronic configuration

A
29
Q

Learn how to write orbital box notation

A
30
Q

What provides evidence for the electronic configurations of sub shells

A

First, second and subsequent ionisation energies with increasing atomic number for the first 36 elements can be explained in terms of the relative stability of different subshell electronic configurations

31
Q

The more stable the electronic configuration

A

The higher the ionisation energy

32
Q

Whats the ionisation energy

A

The energy involved in removing one mole of gaseous atoms from one mole of atoms in the gaseous state

33
Q

What generally happens to ionisation energy across a period

A

Increases as electrons are being removed from the same shell and the nucleur charge increases along the period and so the outer electrons experience greater attraction.

34
Q

Why isn’t there a constant increases in ionisation energy across a period from group 2 to 3

A

The added electron is in the new p subshell which has a slightly higher energy level and is slightly further from the nucleus. The s2 electrons also provide shielding of group 3 elements

35
Q

Why isn’t there a constant increase in ionisation energy from group 5 to 6 and period 3

A

Due to the stability of the p orbitals

36
Q

The more stable the electronic configuration present the what

A

The harder it is to remove the outer electron from its attraction to the nucleus and the higher the ionisation energy

37
Q

What bits of the periodic table have what blocks

A

Hydrogen, helium and first two columns have s blocks
Transition metals have d blocks
Bottoms bit has f blocks
Right side is p blocks

38
Q

What is a dative covalent bond

A

One in which one atom of the bond provides both electrons of the bonding pair

39
Q

What are lone pairs

A

Non bonding electron pairs

40
Q

Describe pairs of electrons

A

They are negatively charged and so repel each other. Arranged in a way so they are as far apart as possible so repulsion is minimised

41
Q

What is VSEPR theory used for

A

To predict the shapes of molecules and poly atomic ions

42
Q

What is the arrangement of electron pairs

A

Linear, trigonal, tetrahedral, trigonal bipyramidal, and octahedral

43
Q

Whats the order of decrease in electron pair repulsion’s

A

Lone pair-lone pair, lone pair-bonding pair, bonding pair-bonding pair

44
Q

When is a covalent bond formed

A

When two atomic orbitals combine together to form a molecular orbital

45
Q

What’s the number of electron pairs formula

A

Number of electron pairs= (electrons of central atom+ number of atoms attached) /2

46
Q

What name is given to each total number of electron pairs

A

2=linear 3=trigonal 4= tetrahedral 5= trigonometry bipyramidal 6= octahedral

47
Q

Whats the number of electron pairs for BrF4 -

A

7 central atoms + 1 charge electron (for the negative and - if it was positive) + 4 atoms attached divided by 2

48
Q

Describe lone pairs

A

Held closer to the central atom so they have greater repulsion than the bonding pairs of electrons

49
Q

Learn bi=one angles for tetrahedral, pyramidal and angular shapes

A
50
Q

What do lone pairs do to bond angles in tetrahedral

A

Cause it to decrease by 2.5 degrees for each lone pair

51
Q

Describe electrons

A

Behave as standing waves in an atom. These are waves that vibrate in time but do not move in space

52
Q

Whats can be explained by considering the electronic configurations

A

Anomalies in the trends of ionisation energies can be explained by considering the electronic configuration

Chemistry Unit 1 How To Pass Book (3 decks)

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