Week One Flashcards by Yasmin bishop

Atom

Chemical species with a central positively charged nucleus surrounded by negatively charged electrons

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Free Atoms

Usually unstable

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Molecules

Atoms with definite structure held together by chemical bonds

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Molecules- electrical

Electrically neutral therefore uncharged

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Covalent bonds

Sharing electrons between neighbouring atoms

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Ions

Species that are either positively or negatively charged

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Cations

Positively charged

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Anions

Negatively charged

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Compounds

Substances containing one or more molecules

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Law of conservation of mass

No gain or loss occurs in chemical reactions, mass is conserved

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Law of Definite proportions

In chemical compounds, elements are always combined in the same proportion by mass

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Law of multiple proportion

When 2 elements form one or more compound, the different masses of one element that combine with the same mass of the other element are in ratio of small whole numbers

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Daltons Atomic Theory

Matter consists of particles
Atoms are indestructible
Atoms of different elements differ in mass and properties

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F block elements

Bottom two rows of periodic table

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D block elements

Groups 3-12

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S block elements

Groups 1-2

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P block elements

Groups 13-18

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Metals - properties

Good conductors of heat and electricity
Malleable
Ductile
Metallic lustre

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Nonmetals - properties

Poor conductors of heat and electric 
Not malleable
Not ductile 
No metallic lustre
Majority are gases at room temp

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Metalliods - properties

Tend to be semi conductors

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Excited state of electrons

Electron lies further from the nucleus, can be promoted to this state by absorption of energy

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Redox reactions

Reactions in which one or more electrons are transferred between chemical species

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Ground state

Lowest energy arrangement of electrons in the orbital

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Pure substances

Have distinct composition and properties

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Homogenous Mixtures

Can be solutions, consistent throughout, can't distinguish individual regions

Heterogeneous mixtures

Composition varies through, consists of two or more identifiable regions

Solids

Ordered arrangements, particles close together, low temp high pressure

Liquid

Disordered wit particles free to move while remaining in close contact (intermediate temp and pressure)

Gas

Total disorder, much empty space, intermolecular forces broken (high temp low pressure)

Physical change

Reversible

Chemical change

Irreversible

Chemical property

Ability to undergo chemical change

Physical property

Involves change in form but not chemical identity

Isotopes

Same number of protons and electrons but different number of neutrons so different mass number

Periods

Horizontal rows

Groups

Vertical rows

0 degrees

273.15 kelvin

Exact numbers

Come from defined values or from counting objects

Imexact numbers

Comes from measurement as there are always limitations

Percentage uncertainty

(Absolute uncertainty/ measured quantity) x 100

Significant figures - + and -

Result has same number of decimal places as the measurement with the fewest number of decimal places

Significant numbers - x and /

Same number of significant figures as the measurement with the least figures

Molecular Formalue

Chemical formula that refers to discrete molecule

Naming - ionic compounds

Cation followed by anion

Covalent compounds

Carbon first, followed by hydrogen then remaining elements in alphabetical order

Naming - inorganic compounds

Element closest to the left of periodic table appears first | First element retains elemental name, second element has suffix ide

Oxoanions

Root name from central atom

Oxoanion with fewer molecules when 2 different

-ire

Oxoanions with more atoms S uffix when 2 different oxoanions

-ate

Alcohol

Functional group + oxygen + hydrgon

Aldehydes

Functional group+ carbon=oxygen + hydrogen

Ketone

Functional group+ carbon=oxygen + functional group

Carboxylic Acids

Functional group + carbon=oxygen+ OH

First she'll

2 electrons

Second she'll

Up to 8 electrons

Third she'll

Up to 18 electrons

Forth and other shells

Up to 32 electrons

Covalent bond - energy

Very strong bonding so it takes a lot of energy to break

Ionic attraction

Attraction of opposite charges

Hydrogen bonds

Attraction between h+ and strongly electronegative atom

Hydrophobic interactions

Interactions of non polar substances in the presence of polar substances

Van der waals interactions

Interaction of electrons of non polar substances

Sharing of electrons covalent bonds

If 2 of same atom then sharing is equal | If 2 different atoms then sharing isn't equal and the one with the greater force will hold electrons closer

Week One Flashcards

(63 cards)