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Grade 11 Chemistry > Matter unit > Flashcards

Matter unit Flashcards

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1
Q

Define chemistry

A

The study the composition and properties of matter

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2
Q

Define Matter

A

Any substance that has mass and has volume (occupies space)

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3
Q

What is all matter composed of

A

Atoms

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4
Q

Charge, atomic mass, and symbol of protons

A

+ charge , 1u atomic mass unit, p+

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5
Q

Charge, atomic mass, and symbol of neutron

A

Neutral charge, 1u (atomic mass unit) , n0

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6
Q

Charge, atomic mass, and symbol of electrons

A

Negative charge, 1/2000 u (atomic mass unit), n-

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7
Q

Where are protons and neutrons contained

A

In the nucleus

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8
Q

Where are electrons found

A

In orbit around the nucleus

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9
Q

Define molecules

A

2 or more atoms bonded together
Hofbrincle can be the same element

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10
Q

Define properties

A

Characteristics that help describe and identify matter

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11
Q

Define Physical property

A

Can be observed without changing one kind of matter into something new. Ex Colour texture odours lustre

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12
Q

Define Chemical property

A

Observed when one kind of matter is converted into a different kind of matter. Ex mg produced hydrogen gas in acid.

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13
Q

Define qualitative

A

Can be described in words but cannot be measured or expressed with numbers

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14
Q

Define quantitative

A

Can be measured and expressed with numbers

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15
Q

Physical changes

A

Affect the physical appearance of matter,but not it’s composition. (Change in physical properties only)

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16
Q

Chemical change

A

Changes that alter the composition of matter (change in both physical and chemical properties

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17
Q

The 5 Clues for a chemical change

A

Colour change
Production of gas (bubbles)
Precipitate (solid) formation
Heat absorbed or released
Light produced

18
Q

Bohr Rutherford vs Louis dot

A

Bohr Rutherford shows all electrons and the protons and neutrons in the nucleus where as Louis dot diagram shows valence electrons

19
Q

The periodic law

A

The periodic law states that the properties of elements repeat in a pattern when they are arranged by atomic number

20
Q

Groups in the periodic table

A

Alkali metals
Alkaline earth metals
Halogens
Noble gases
Transition metals

21
Q

Properties of metals

A

Shiny
Solid (most)
Malleable
Ductile
High Conductive

22
Q

Properties of metalloids

A

Some shiny some not
Solids
Brittle
Not ductile
Semi conductor

23
Q

Non metals

A

Not shiny
Brittle
Mostly gases
Not ductile
Not conductive (insulators)

24
Q

Reactivity

A

How easily and quickly elements react(combine)

25
Q

Reactivity of metals

A

Reactivity of metals goes down as you go right across the periodic table

26
Q

reactivity of non metals

A

The reactivity of non metals increases going left (not including noble gases)

27
Q

Isotopes

A

Isotopes are atoms that have the same number of electrons and protons but a different number of neutrons (same atomic number different atomic mass)

28
Q

Radio isotopes

A

Isotopes with unstable nuclei that release high energy particles when they break apart

29
Q

Average atomic mass

A

Weighted average of the atom masses and abundance

30
Q

Atomic radius

A

The size of an atomic (measured from the nucleus to the outer edges of the cloud like outer edges of the atom)

31
Q

Atomic radius pattern and reason behind it

A

Atomic radius increases going down the periodic table as there are more energy shells that make the valence electrons further from the nucleus and lowers the effective charge of nucleus as it’s blocked by the other shells

Atomic radius increases going right as the valence electrons are on the same energy level however the charge of the nucleus is higher which pulls the valence electrons closer

32
Q

Ionic compounds

A

Ionic compounds are formed between a non metal and a metal, when the metal transfers its valence electrons to the mon metal. This results in the positively charged metal ion (cation) and negatively charged non metal ion(anion), which are attracted and form a bond

33
Q

Covalent bonds

A

Are between non metals, and occurs when they share electrons to get a full shell

34
Q

Ionic compound properties

A

Solid at room temp
Hard
High melting and boiling points
High solubility in water
Conductive in water and as a liquid

35
Q

Covalent bonds properties

A

Can be solid liquid or gas at room temp
Soft
Low melting and boiling point
Usually low solubility in water
Not conductive

36
Q

Diatomic elements

A

Hydrogen
Bromine
Fluorine
Chlorine
Iodine
Oxygen
Nitrogen

37
Q

Covalent compound prefixes

A

Mono
Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca

38
Q

Common names

A

H20 - water
NH3 - ammonia
CH4 menthane
H2S hydrogen sulphide

39
Q

Polyatomic ions

A

Poly atom ions are treated as normal ions in a compound

40
Q

Key oxyions

A

No3-1
So4-2
Po4-3
Co3-2
Clo3 -1
Io3-1
Bro3-1

41
Q

OxyContin change in name

A

+1 oxygen - pernitrate NO4 -1
Keyoxyion - nitrate NO3 -1
- 1 oxygen - nitrite NO2 -1
-2 oxygen - hyponitrite NO -1

42
Q

Oxyacids

A

Oxyions change
ate to ic
It’s to ous

Grade 11 Chemistry (5 decks)

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