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Chemistry > Utt Module 1 > Flashcards

Utt Module 1 Flashcards

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1
Q

Define matter

A

Anything that occupies space(has volume) and has mass

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2
Q

What is matter made up of

A

a substance made of elements which have specific physical properties and cannot be broken down into simple substances

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3
Q

how much elements are there and how much are natural

A

118 element only 92 are natural and the others are made in labs and are unstable

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4
Q

Define the term atom

A

An atom is the smallest, identifiable unit of matter that retains all of the chemical properties of an element

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5
Q

What are the subatomic particles of an atom

A

proton
electron
neutron

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6
Q

What is the relative charge of a proton

A

+1

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6
Q

How are the subatomic particles arranged in the atom

A

the protons and neutrons are grouped together in the nucleus while the electrons orbit around the nucleus on the shells.(travel around the nucleus in circular orbits

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7
Q

what is the relative charge of an electron

A

-1

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8
Q

what is the relative charge of a neutron

A

0

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9
Q

what is the relative mass of a proton

A

1

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10
Q

what is the relative mass of a neutron

A

1

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11
Q

what is the relative mass of an electron

A

negligible
1/1840

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12
Q

Define atomic number of an atom

A

the number of protons in an element

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13
Q

What is the atomic number denoted by

A

Z

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14
Q

What is another name for atomic number

A

proton number

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15
Q

The number of protons is equal to the

A

atomic number and number of electrons

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16
Q

the number of electrons in an atom is equal to

A

the number of protons

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17
Q

define electrically neutral

A

has no net charge therefore the number of proton and electrons are neutral

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18
Q

define the mass number of an atom

A

the total number of protons and neutrons in an atom

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19
Q

The mass number is denoted by

A

A

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20
Q

Explain the periodic table notation of an atom

A

the atomic number is at the top left of the periodic tile
the element symbol is at the center with the name below
the atomic weight is
the average atomic mass is under the name
ZA

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21
Q

Explain the nuclear notation of an atom

A

A
X
Z
The element’s symbol is at the center with the mass number at the top and the atomic number below
AZ

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22
Q

What is the nucleon number of an atom

A

the mass number which is the number of protons and neutrons in an atom

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23
Q

How is the periodic table arranged

A

the atomic number increases horizontally therefore if reading in the order of the number of protons you read it horizontally. Also the period increases every row whilst the group increases every column

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24
Q

list the first 30 elements of the periodic table

A

Hydrogen
Helium
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
Sodium
Magnesium
Aluminium
Silicon
Phosphorus
Sulphur
Chlorine
Argon
Potassium
Calcium
Sodium
Magnesium
Aluminium
Silicon
Phosphorus
Sulphur
Chlorine
Argon
Potassium
Calcium

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25
Q

First 10 elements of the periodic table

A

Hydrogen
Helium
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon

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26
Q

Second 10 elements in the periodic table

A

Sodium
Magnesium
Aluminium
Silicon
Phosphorus
Sulphur
Chlorine
Argon
Potassium
Calcium

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27
Q

Third 10 elements of the periodic table

A

Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc

28
Q

How to remember the second 10 element in the periodic table

A

SMASP(smash with a p at the end instead of h)
SCAKC (scake with c at the end instead of e)

29
Q

How to remember the first the third 10 element

A

Scent Tinted Vase Cried Marol Fendi the Cobra Niece bit Cute Zian

30
Q

Sliver symbol, atomic number and mass number

A

Symbol:Ag
Atomic Number: 47
Mass Number: 108

31
Q

Gold symbol atomic number and mass number

A

Symbol: Au
Atomic Number: 79
Mass Number: 198

32
Q

What 5 things can you get from the nuclear notation of a chemical

A

Atomic Number
Mass Number
Number of Protons
Number of Electrons
Number or Neutrons

33
Q

Define isotope …Therefore

A

An isotope is the different forms of element with the same number of protons but different number of neutrons.
Therefore it has they have the same atomic number but different mass number

34
Q

Give four examples of naturally occurring isotopes

A

Carbon 12 13 14
Potassium 39 40 41
Uranium 238 235
Chlorine 35 37

35
Q

What are the Hydrogen Isotopes

A

Hydrogen-1 Protium
Hydrogen-2 Deuterium
Hydrogen-3 Tritium

36
Q

Since not all atoms of a given element has the same number of neutrons we calculate

A

the averaged mass called RAM

37
Q

what does R.A.M. stand for

A

Relative Atomic Mass

38
Q

How do you calculate RAM

A

RAM= ∑(masse x abundance)

39
Q

What do you need to calculate RAM

A

the mass of the isotope
The abundances (usually %) of the isotopes.

40
Q

When calculating RAM don’t forget to

A

divide percentages by 100
include units ie amu

41
Q

what is RAM units

A

amu

42
Q

What does Bohr Model Tell us

A

electrons travel around the nucleus in circular orbits. the electrons in the Bohr model could orbit only at specific fixed distances from the nucleus.

43
Q

when the electron moves from an outer shell to an inner shell it… the equation for this is

A

looses energy since it requires more energy to hold it in the outer shell. the equation for this is △E=hv

44
Q

The Pauli exclusion principle suggests that

A

only two electrons with opposite spin can occupy an atomic orbital

45
Q

Hund’s rule suggests that

A

electrons prefer parallel spins in separate orbitals of subshells. This rule guides us in assigning electrons to different states in each sub-shell of the atomic orbitals. In other words, electrons fill each and all orbitals in the subshell before they pair up with opposite spins

46
Q

what determines the group of an element in the period table

A

the number of valance electrons

47
Q

what determines the period of an element in the period table

A

the number of shells

48
Q

Valence Electron definition

A

Valence electrons are electrons in the outermost shell of an atom, and that can participate in the formation of a chemical bond with other atoms

49
Q

what are the advantages of grouping elements in the periodic table

A

Identification
Properties
Classifications

50
Q

Properties of metals

A

shiny
good conductors of heat and electricity
bend without breaking
solid at room temp
hard and strong
malleable
high density
makes a ringing sound when hit

51
Q

Properties of non-metals

A

dull
doesn’t make a ringing sound when hit
weak and brittle
low density
poor conductors of heat and electricity

52
Q

Metalloid properties

A

two main criteria behaves similar to semiconductors and often creates amphoteric oxides
solid at room temperature
some are good conductors under the write conditions like silicon and germanium when doped

53
Q

Define valency

A

a measure of an elements combining power with other atoms when it forms chemical compounds or molecules

54
Q

How is valency measured

A

the combining power or affinity of an atom of an element was determined by the number of hydrogen atoms that it combined with.

55
Q

Define Cation

A

A cation is a positively charged ion and is formed when an atom loses one or more electrons

56
Q

Define Anion

A

An anion is negatively charged and is formed when an atom gains one or more electrons

57
Q

What are the three types of primary bonding

A

Ionic
Metallic
Covalent

58
Q

Define chemical bond

A

attraction between atoms that allows the formation of chemical substances that contain two or more atoms.

59
Q

Define ionic bonding

A

Electrons are transferred from one atom to another resulting in the formation of positive and negative ions

60
Q

ionic bonding includes

A

a metal and a non metal

61
Q

metals in ionic bonding from

A

positive ions

62
Q

non metals in ionic bonding form

A

negative ions

63
Q

covalent bonding

A

a form of chemical bonding characterized by the sharing of pairs of electrons between atoms, and other covalent bonds

64
Q

Ionic bonds form when

A

a metal reacts with a non-
metal

65
Q

Covalent bonding only occurs between

A

non-metals

66
Q

Ionic…Covalent…

A

Ionic gives Covalent shares

67
Q

Metallic Bonding is

A

Metallic bonding is the strong attraction between closely packed positive metal ions and a ‘sea’ of delocalized electrons

Chemistry (8 decks)

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