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Utt Module 1 Flashcards

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 are in the orbits surrounding the nucleus.

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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
list the first 30 elements of the periodic table
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
25
First 10 elements of the periodic table
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
26
Second 10 elements in the periodic table
Sodium Magnesium Aluminium Silicon Phosphorus Sulphur Chlorine Argon Potassium Calcium
27
Third 10 elements of the periodic table
Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc
28
How to remember the second 10 element in the periodic table
SMASP(smash with a p at the end instead of h) SCAKC (scake with c at the end instead of e)
29
How to remember the first the third 10 element
Scent Tinted Vase Cried Marol Fendi the Cobra Niece bit Cute Zian
30
Sliver symbol, atomic number and mass number
Symbol:Ag Atomic Number: 47 Mass Number: 108
31
Gold symbol atomic number and mass number
Symbol: Au Atomic Number: 79 Mass Number: 198
32
What 5 things can you get from the nuclear notation of a chemical
Atomic Number Mass Number Number of Protons Number of Electrons Number or Neutrons
33
Define isotope ...Therefore
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
Give four examples of naturally occurring isotopes
Carbon 12 13 14 Potassium 39 40 41 Uranium 238 235 Chlorine 35 37
35
What are the Hydrogen Isotopes
Hydrogen-1 Protium Hydrogen-2 Deuterium Hydrogen-3 Tritium
36
Since not all atoms of a given element has the same number of neutrons we calculate
the averaged mass called RAM
37
what does R.A.M. stand for
Relative Atomic Mass
38
How do you calculate RAM
RAM= ∑(masse x abundance)
39
What do you need to calculate RAM
the mass of the isotope The abundances (usually %) of the isotopes.
40
When calculating RAM don't forget to
divide percentages by 100 include units ie amu
41
what is RAM units
amu
42
What does Bohr Model Tell us
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
when the electron moves from an outer shell to an inner shell it... the equation for this is
looses energy since it requires more energy to hold it in the outer shell. the equation for this is △E=hv
44
The Pauli exclusion principle suggests that
only two electrons with opposite spin can occupy an atomic orbital
45
Hund's rule suggests that
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
what determines the group of an element in the period table
the number of valance electrons
47
what determines the period of an element in the period table
the number of shells
48
Valence Electron definition
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
what are the advantages of grouping elements in the periodic table
Identification Properties Classifications
50
Properties of metals
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
Properties of non-metals
dull doesn't make a ringing sound when hit weak and brittle low density poor conductors of heat and electricity
52
Metalloid properties
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
Define valency
a measure of an elements combining power with other atoms when it forms chemical compounds or molecules
54
How is valency measured
the combining power or affinity of an atom of an element was determined by the number of hydrogen atoms that it combined with.
55
Define Cation
A cation is a positively charged ion and is formed when an atom loses one or more electrons
56
Define Anion
An anion is negatively charged and is formed when an atom gains one or more electrons
57
What are the three types of primary bonding
Ionic Metallic Covalent
58
Define chemical bond
attraction between atoms that allows the formation of chemical substances that contain two or more atoms.
59
Define ionic bonding
Electrons are transferred from one atom to another resulting in the formation of positive and negative ions
60
ionic bonding includes
a metal and a non metal
61
metals in ionic bonding from
positive ions
62
non metals in ionic bonding form
negative ions
63
covalent bonding
a form of chemical bonding characterized by the sharing of pairs of electrons between atoms, and other covalent bonds
64
Ionic bonds form when
a metal reacts with a non- metal
65
Covalent bonding only occurs between
non-metals
66
Ionic...Covalent...
Ionic gives Covalent shares
67
Metallic Bonding is
Metallic bonding is the strong attraction between closely packed positive metal ions and a 'sea' of delocalized electrons
68
Why don't solids pass through each other in the have all that space in their shells
Because the negatively charged electron clouds of atoms repel each if they get too close.
69
What number determines the atom we are looking at
The number of protons aka the atomic number
70
What relation do protons have to electrons in an electrically neutral atom?
They are equal to each other
71
What is actually RAM
RAM os the average mass of an elements isotopes

Chemistry (8 decks)

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