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PMP 102 > From Atoms To Molecules > Flashcards

From Atoms To Molecules Flashcards

1
Q

Atomic number is the number of…

A

Protons

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2
Q

Mass number is the number of…

A

Protons and neutrons

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3
Q

Isotopes are…

A

The same number of protons but different number of neutrons.

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4
Q

Cations have more…

A

Protons than electrons

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5
Q

Anions have more…

A

Electrons than protons

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6
Q

Elements are…

A

Atoms of one type

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7
Q

Compounds are…

A

Atoms of two or more different elements join

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8
Q

Molecules are…

A

Atoms that are stuck together

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9
Q

Mole is…

A

Avogadro’s number
6.022x10*23

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10
Q

Molarity is…

A

The number of moles of solute per litre of solution

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11
Q

Relative mass is…

A

The weighted average of all isotopes

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12
Q

Molecular weight is…

A

The mass of a molecule of a substance.

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13
Q

Molar mass is…

A

The mass of one mole of substance

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14
Q

What happens when we go across the periodic table?

A

Atomic size decreases
Number of valence electrons increases
Electronegativity increases
Oxidising nature increases

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15
Q

What happens when we go down the group on the periodic table?

A

Atomic size increases
Number of valence electrons remains the same
Electronegativity decreases
Oxidising nature decreases

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16
Q

What is the definition of organic chemistry?

A

The chemistry of carbon compounds.

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17
Q

What are atomic orbitals?

A

Electrons are grouped into different shells at different distances from the nucleus.

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18
Q

What is the principle quantum number

A

n
Is the number of shells

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19
Q

How many electrons can each shell contain?

A

2n*2

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20
Q

What are the energy levels of the shells?

A

Further from the nucleus has a higher energy level.
As it can hold more electrons.

21
Q

How many and what sub shells are there?

A

4 subshells (s,p,d,f)

22
Q

What shape is the s orbital?

A

Spherical

23
Q

What shape is the p orbital?

A

Two slim spheres on top of each other.

24
Q

What shape is the d orbital?

A

4 long tear drop shapes attached at their tails, equally separated.

25
Q

What shape is the f orbital?

A

8 tear drop shapes attached at their tails separated equally (360)

26
Q

How many orbitals does the s subshell contain?

A

1

27
Q

How many orbitals does the p subshell contain?

A

3

28
Q

How many orbitals does the d subshell contain?

A

5

29
Q

How many orbitals does the f subshell contain?

A

7

30
Q

The definition of electronic configuration of atoms is…

A

The number of electrons that an atom possesses, and the orbitals in which those electrons are placed in.

31
Q

What are the valance electrons?

A

Electrons on the outer most shells.

32
Q

The definition of valence is…

A

The number of electrons an atom must lose or gain to attain the nearest noble gas.

33
Q

What is the Aufbau Principle of ground-state electronic configuration?

A

Orbitals and shells fill in order of increasing energy.

34
Q

What is the Pauli Exclusion Principle of ground-state electronic configuration?

A

Each atomic orbital can hold a maximum of 2 electrons.

35
Q

What is the Hunds rule for ground-state electronic configuration?

A

When there are 2 or more orbitals of the same energy, electrons go in different directions.

36
Q

What is the octet rule?

A

Atoms transfer or share electrons to attain a filled shell of electrons (noble gases).

37
Q

What is ionic bonding?

A

Transferring electrons from one atom to another.
Ions have opposite charges, and they attract each other to form an ionic bond.

38
Q

Covalent bonding is…

A

Electrons are shared rather than transferred.

39
Q

Non-polar covalent bonds is when…

A

Electrons are shared equally.

40
Q

Polar covalent bonds are…

A

Unequally shared pair of bonding electrons.

41
Q

What is the definition of electronegativity?

A

Power of an atom in a molecule to attract electrons to itself.

42
Q

What is the definition of bond polarity?

A

The amount of partial charge multiplied by the bond length.

43
Q

The 3 different types of intermolecular forces are…

A

1) dipole-dipole interactions
2) van der walls forces
3) hydrogen bonding

44
Q

What is a dipole-dipole interaction?

A

Interactions between the positive end of one dipole and the negative end of another dipole.

45
Q

What are van der walls forces?

A

Relatively weak forces of attraction that exist between non polar molecules.

46
Q

What is hydrogen bonding?

A

Attractive force between the H attached to an electronegative atom of one molecule and an electronegative atom of the same or different molecule.

47
Q

sp3 hybridisation is…

A

C forms 4 single bonds

48
Q

sp2 hybridisation is…

A

C forms a double bond

49
Q

sp hybridisation is…

A

C forms a triple bond or accumulate double bond.

PMP 102 (29 decks)

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