Atomic structure and the periodic table Flashcards

1
Q

What is an atom?

A

The smallest part of an element that can still be recognised as that element

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2
Q

What is a compound?

A

•A substance made when two or more elements are chemically bonded together.
•Can only be separated into elements by chemical reactions

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3
Q

What is a mixture?

A

•When some elements or compounds are mixed together but do not react together
•Impure substance

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4
Q

How can mixtures be separated?

A

Physical process e.g
•Filtration
•Crystalisation
•Fractional distilation
•Chromotograhy
•Simple distillation

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5
Q

What is the relative charge of a proton?

A

+1

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6
Q

What is the relative charge of a neutron?

A

0

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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 mass of a proton?

A

1

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9
Q

What is the relative mass of a neutron?

A

1

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10
Q

What is the relative mass of an electron?

A

very small

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11
Q

Describe the nucleus of an atom?

A

*in the middle of the atom
*contains protons and neutrons
*positive charge due to protons
*almost whole mass of atom is concentrated at the atom

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12
Q

Describe the electrons of an atom?

A

•move around in electron shells
•negatively charged
•have virtually no mass

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13
Q

Why do atoms have no overall charge?

A

The number of electrons is equal to the number of protons in the nucleus

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14
Q

What is the atomic number of an atom?

A

the number of protons it contains

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15
Q

What is the mass number of an atom?

A

The bigger number, the sum of the protons and neutrons

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16
Q

What is the relative atomic mass of an atom?

A

An average value that takes into account the abundance of the isotopes of the element.

17
Q

Describe the electronic structure of an atom?

A

maximum 2 electrons in the first shell
maximum 8 in the second shell
maximum 8 in the third shell

18
Q

What was Daltons theory of the atom?

A

solid sphere made up of different elements

19
Q

What was JJ Thomspons theory of the atom?

A

*developed Daltons theory
*plum pudding model
*atoms were positive sphere of charge embedded with electrons

20
Q

What was Rutherford’s theory of the atom?

A

*disproved Thompson’s theory
*conducted the alpha particle scattering experiments
*fired positively charged alpha particles at sheet of golf
*expected particles to pass straight through
*some were defected more than expected and some were deflected backwards
*concluded tiny charged nucleus at the center with a cloud of negative electrons

21
Q

What was Bohr’s theory of the atom?

A

*modern nuclear model
*electrons orbit fixed shells
*further experiments by rutherford showed nucleus divided into smaller particles called protons
*James chadwick proposed the idea of neutral particles called protons also in the nucleus

22
Q

How are elements in the periodic table arranged?

A

*In order of atomic number
*Elements in the same group have the same number of electrons in their outer shell, giving them similar properties

23
Q

Explain the development of the periodic table.

A

*arranged by atomic weights before discovery of protons
*Mendeleev left gaps for elements he thought had not been discovered
*elements with properties predicted filled the gaps
*knowledge of isoptopes explained why order of atomic weights was not always correct

24
Q

What is an isotope?

A

Same number of protons but different number of neutrons

25
Q

What is a metal?

A

An element that reacts to form a positive ion

26
Q

What is a non-metal?

A

An element that do not form positive ions

27
Q

Where are metals found in the periodic table?

A

On the left

28
Q

Where are non metals found on the periodic table?

A

On the right

29
Q

What are some properties of metals?

A

*Theyre strong but malleable
*Great at conducting heat and electricity
*Have high boiling and melting points

30
Q

What are some properties of non metals?

A

*More brittle
*Aren’t always solids
*don’t generally conduct electricity
*often have a lower density

31
Q

Describe group 0 elements.

A

*Called noble gasses
*Unreactive so do not easily form molecules as have stable arrangements of electrons
*Have 8 electrons in outer shell except helium which has 2
*Boiling points increase going down the group

32
Q

Describe group 1 elements.

A

*Alkali metals
*1 electron in their outer shell
*Reactivity increases going down the group.

33
Q

How do the first 3 elements of group 1 (Lithium, Sodium, Potassium) react with water?

A

*React vigorously to produce hydrogen gas and metal hydroxides
*The more reactive (lower down the group) more violent reaction is
*Amount of energy given out by reaction increases going down the group.

34
Q

How do the first 3 elements of group 1 (Lithium, Sodium, Potassium) react with Chlorine?

A

*React vigorously when heated in chlorine gas to form white metal chloride salts
*Reaction more vigorous as you go down the group

35
Q

How do the first 3 elements of group 1 (Lithium, Sodium, Potassium) react with Oxygen?

A

*React with oxygen to form metal oxide

36
Q

Describe group 7 elements.

A

*Known as halogens
*Non-metals and consist of molecules made of pairs of atoms
*Form ionic bonds with metals
*Form covalent bonds with non-metals

37
Q

What are the physical properties of transition metals?

A

•conduct electricity
• shiny when freshly cut
• high melting points
• high densities
• greater strength
• greater hardness

38
Q

What are chemical properties of transition metal?

A

• react slowly with oxygen and water or not at all
• some react with halogens
• form ions with different charges
• form coloured compounds
• good catalysts