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Chemistry > Review > Flashcards

Review Flashcards

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1
Q

5 clues a chemical reaction occurred

A 
Gas or odour released
Colour change
Precipitate
Temperature change
Light released
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2
Q

Law of conservation of mass

A

The mass of the reactants is the same as the mass of the products

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3
Q

First ionization energy

A

The energy required to remove an electron from an atom at its ground state

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4
Q

Trends ionization energy and electro negativity

A

Decreases as we go down a group

Increase from left to right

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5
Q

Trends atomic radius

A

Increases going down a group

Decreases going across a period

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6
Q

Proton symbol charge and mass

A

P+ +1 charge 1.674 x 10^-24

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7
Q

Neutron symbol charge and mass

A

n neutral 1.67 x 10 ^-24

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8
Q

Electron symbol charge and mass

A

e- -1 9.1094 x 10^-28

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9
Q

Stages of development of atomic theory

A

Dalton billiard ball model
Thompson plum pudding
Rutherford beehive
Bohr-quantum

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10
Q

Dalton Model

A

Billiard ball

All atoms of the same element are the same size. Each element has a different size.

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11
Q

Thompson

A

Plum pudding

Aaron’s are solid positive balls with negative electrons embedded throughout it. It’s still neutral

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12
Q

Rutherford

A

Beehive
Atom is mostly empty space. Most of the mass is in the nucleus. Electrons move around nucleus like planets around the sun

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13
Q

Bohr

A

Quantum
Electrons travel around nucleus in specific energy levels. Atoms get excited and absorb energy and boost to a higher level. Then they drop to the ground state and release light

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14
Q

Isotope

A

When an atom has the same number of protons but a different number of neutrons

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15
Q

Average atomic mass

A

The sum of the masses of isotopes each multiplied by its natural abundance on earth. Basically the average mass of the element on earth

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16
Q

What is Bohrs theory based on?

A

He directed light through a prism with a screen behind it. Then lines of certain colour shot through. Hydrogen is unique and doesn’t have all the colours as everyone else.

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17
Q

Ground state

A

All the electrons are in the lowest possible energy levels

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18
Q

Excited state

A

The energy in an atom is higher than that in the ground state.

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19
Q

Pauli exclusion principle

A

Only 2 electrons of opposite spin can occupy one orbital

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20
Q

Aufbau principle

A

Building up. Each electron occupies the lowest energy orbital available

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21
Q

Hunds rule

A

All electrons in single occupied orbitals spin the same way.

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22
Q

Covalent bonds

A

Bond that results from sharing of a pair of electrons by 2 atoms.

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23
Q

Polar covalent bonds

A

A covalent bond formed between atoms with significantly different electronegativities resulting in a molecule with localized charges.

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24
Q

Ionic bond

A

The electrostatic force of attraction between a positive ion and a negative ion bond them together

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25
Q

Three types of intermolecular forces

A

Dipole dipole forces
London dispersion forces
Hydrogen bonds

26
Q

Dipole dipole forces

A

Van see Waals force. And attractive force between polar molecules. The positive end of one molecule is attracted to the negative end of one molecule

27
Q

London dispersion forces

A

Van get Waals force

Weak attractive force acting between all atoms

28
Q

Hydrogen bonds

A

Strongest attraction.

29
Q

Polar molecules

A

A molecule that is slightly positively charged and slightly negatively charged at the other end due to electronegativity differences

30
Q

Non polar molecules

A

The electrons are equally distributed among the atoms resulting in no localized charging

31
Q

Products of combustion of a hydrocarbon

A

Co2 and h2o

32
Q

Properties of metals

A

Shiny solid good conductors high melting points low electronegativity a lot of lister

33
Q

Properties of non metals

A

Dull. Solids liquids and gases. Low density brittle. Poor conductors. No lister

34
Q

Atomic number

A

The unique number of protons in one atom of an element.

35
Q

Mass number

A

The weighted average of all the naturally occur in isotopes of an element

36
Q

How do you find the number of neutrons

A

Mass#-atomic#

37
Q

How do you know the protons

A

It’s the atomic number. As well as the number of electrons

38
Q

Group

A

A column of elements in the periodic table. Up and down

39
Q

Family

A

Same as group

40
Q

Period

A

A row on the periodic table of the elements. Left to right

41
Q

Alkali metals

A

1st column on periodic table most reactive metal

42
Q

Alkali earth metals

A

2nd column. Pretty reactive metals

43
Q

Mettaloids

A

Have properties of metals and non metals

44
Q

Transition metals

A

From row 3 to 13. The d orbital

45
Q

Rare earth metals

A

Lanthanides and actinides. Below the periodic table

46
Q

Noble gases

A

Column 18 full valence electrons

47
Q

Halogens

A

Most reactive gas column 17

48
Q

Where is the s block located

A

Group 1 and 2 and helium

49
Q

Where is the p block located

A

Group 13-18

50
Q

Where is the d block located?

A

Transition metals. Group 3-12

51
Q

Where is the f block located?

A

Lanthanides and actinades below the table

52
Q

Isoelectronic

A

When it has the same number of electrons as a noble gas

53
Q

Reactivity of metals

A

The tendency metals have of losing electrons.
Increases going down. Decreases from left to right.
More energy levels so electrons can be pulled away easier

54
Q

Reactivity of non metals

A

The tendency of a non metal to gain electrons.
Decreases going down. Increases left to right.
Because less energy levels means more attraction

55
Q

Electronegativity

A

The tendency for an atom to attract electrons to itself when it’s chemically combined with another element

56
Q

Which elements form ionic compounds?

A

Metal cations and nonmetal anions

57
Q

Which elements form covalent bonds?

A

Non metals sharing electrons

58
Q

Characteristics of ionic compounds

A

High melting and boiling points. Solids at room temperature. Conductive of electricity in aqueous solution. Crystalline structures

59
Q

Characteristics of covalent bonds

A

Low melting and boiling points. Solid liquid or gas at room temperature. Non conductive of heat or electricity. Non crystalline

60
Q

What does the period number refer to?

A

The number of energy levels

61
Q

What does the group number refer to!

A

of valence electrons

Chemistry (3 decks)

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