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Brainscape Exam Flashcards

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1
Q

Relative mass of protons, neutrons and electrons

A

Protons:1
Electrons:0.0005
Neutrons:1

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2
Q

Octet rule

A

2,8,18,18,8

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3
Q

Valence electrons

A

Electrons which are lost or gained to form ions or are shared to form bonds

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4
Q

Electrons always fill from

A

Lowest energy to highest energy t/f first shell fills first

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5
Q

Isotopes

A

Same number of protons, different numbers of neutrons

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6
Q

Atomic radii

A

Total distance from the nucleus of an atom to the outermost orbital of its electron

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7
Q

Ionic bonding is

A

Intramolecular bonding (within molecules)

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8
Q

Giant meaning in giant ionic lattice

A

Undefined number of particles in lattice

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9
Q

Why are ionic compounds brittle

A

Giant ionic lattice. Each negatively charged ion is surrounded to a positively charged ion. This arrangement forms layers within the lattice. Lattice arrangement of ions that a when a strong enough force is applied, layers may shift causing like charges to align and repel. This breaks the lattice

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10
Q

Monatomic ions

A

Ion formed from a single atom

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11
Q

Poly atomic ions

A

Group of atoms covalently bonded together but group of atoms as a whole has a charge

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12
Q

What does metallic mean in giant metallic lattice

A

Particles are cations and delocalised valence electrons

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13
Q

Alloys

A

Mixtures of two or more metal elements. Cations are different sizes, so when there is a mix of different cation in the G.I.L, layers become disrupted

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14
Q

Alloy are

A

Stronger, harder and less malleable metals than pure metals. When force or stress is applied the layers of cations can no longer slide past each other easily

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15
Q

Why is melting point low for simple covalent molecules

A

There are intermolecular forces between simple covalent molecules. These intermolecular forces are much weaker than string covalent bonds.

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16
Q

When one nucleus has a stronger pull on a shared pair of electrons, the electrons will

A

Sit closer to nucleus which causes a slight imbalance of charge

17
Q

What does covalent mean in giant covalent lattice

A

Valence electrons are shared between atoms

18
Q

Allotrope

A

Different structural form of the same element in the same state e.g diamond and graphite are allotropes of carbon

19
Q

Diamond

A

Each carbon atom in diamond is covalently bonded to 4 other carbon atoms, leaving no free electrons to move and conduct electricity

20
Q

Graphite

A

Each carbon atom is covalently bonded with three other carbon atoms. This leaves a sea of delocalised valence electrons that are free to move and conduct electricity

21
Q

Why is diamond hard

A

All bonding in diamond is covalent bonding which requires a lot of energy to break

22
Q

Graphite hardness

A

Most of bonding in graphite is covalent bonding which requires a lot of energy to break

23
Q

Why is graphite soft

A

Layers of carbon atoms can slide over each other making graphite soft and slippery. There are only weak intermolecular forces between the layers

24
Q

Why is diamond hard

A

In diamond, the atoms are arranged so that all atoms make 4 strong covalent bonds to other carbon atoms

25
Q

Intramolcular

A

Ionic, metallic, covalent

26
Q

Intermolecular forces

A

Found between all simple covalent molecules. They are weaker forces of attraction that are broken down when covalent molecules change states

27
Q

Dispersion

A

Weakest type of intermolecular bond
Occur between all molecules and atoms due to constant movement of electrons h/w at any instant, may be more electrons at one end of molecule than the other h/w only temporary

28
Q

Dipole dipole forces

A

Attraction between polar simple covalent molecules
Force of attraction between slight negative charge of one molecule and slight positive charge pole of another molecule

29
Q

Hydrogen bonds

A

Extra strong dipole dipole attraction that occurs between H-NOF of one molecule and H-NOF to another molecule

30
Q

Strength of intermolecular fore=ces is determined by

A

Atoms in molecules, electronegative of atoms

More electrons an atom has, the stronger the forces of attraction

31
Q

Ionic compounds are

A

Mostly soluble in water b/c polar solutes dissolve in polar solvents e.g like dissolves like

32
Q

Force of attraction between water molecules and ions is

A

Stronger than the attraction between. Ions t/f ion-dipole force

33
Q

Precipitate

A

An insoluble salt formed from two aqueous reagents.

34
Q

How can precipitate be collected

A

By filteration

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