NUMBAT OER - Open Educational Resources

2. The basic dimensions

The basic dimensions are length, time and mass.

Length

The standard unit of length is the metre, denoted by the symbol m. This and other units do not have a plural abbreviation – 'one metre' is written '1 m' and 'two metres' is written '2 m' (not '2 ms'). Other SI units are multiples or divisions of a metre in factors of ten (see the section on Large and small units). Familiar units of length or distance in this system are the metre, millimetre (1 mm = 0.001 m), centimetre (1 cm = 0.01 m) and kilometre (1 km = 1000 m). Note that when the units are written, they are separated from the value by a space, thus: '1.75 m' not '1.75m'.

Areas are the product of two length measurements (for instance, the length and width of a carpet or lawn). The unit for area is the square metre - m2 (m × m). Larger and smaller units are also used, but note that, for instance, km2 is not a thousand square metres but is a square kilometre (one million square metres).

Likewise, volumes are the product of three length measurements (for instance, length, width and depth of a tank or a swimming pool). The basic unit is the cubic metre - m3 (m × m × m). As with area, larger or smaller units have a particular convention - mm3 is a cubic millimetre and has a volume of one thousand-millionth of a cubic metre.

Volumes of fluids are commonly expressed in litres, where one litre is a thousandth of a cubic metre (also equal to a cubic decimetre, 1 dm3). One millilitre (ml) is equal to one cubic centimetre (cm3), and a cubic millimetre (mm3) is equal to one microlitre (μl).

Time

The standard SI unit of time is the second, denoted by the symbol s. Because our systems of time measurement were established well before the metric system of measurement, and because the second is quite a small unit for common use, we continue to use non-SI units for time in biosciences, such as minutes (1 min = 60 s), hours (1 h = 3600 s), days (1 d = 86 400 s) and years (1 y ~ 31 557 600 s).

Measurements of quantities such as speed, the rate of change of distance with time, are expressed as being 'per second' or 'per hour'. The SI adopts a special notation for this - for instance a speed of five metres per second would be written as '5 m s-1', where the 'm s-1' means 'number of metres divided by number of seconds' (see the section on Compound units). Some older texts may use the format 'm/s' to indicate metres per second, but this should no longer be used.

Where regular events take place, such as the vibration of a violin string or of a tuning fork, the rate of these events is expressed as a frequency. The number of events per second is given the unit of Hertz (symbol Hz), where 1 Hz is one vibration or cycle per second (that is 1 Hz = 1 s-1). We encounter this unit in everyday life in describing sounds and radio waves, where units such as kilohertz (kHz) and megahertz (MHz) are used, and in the clock speeds of computer processors expressed in gigahertz (GHz).

Measurement of radioactivity, as the rate of nuclear disintegrations, is also expressed using a time-based unit. The Bequerel (symbol Bq) is one nuclear disintegration per second, so that 1 Bq = 1 s-1. A decay rate of 1 Bq is so low as to be practically immeasurable, so that you are more likely to encounter the units kilobequerels (1 kBq = 1000 Bq) or megabequerels (1 MBq = 1 000 000 Bq). You may encounter an older non-SI unit, the curie, where 1 Ci = 37 GBq. Because different radioisotopes differ in the type and energy of their emissions, the Bequerel is not a consistent measure of energy intensity or exposure.

Mass

Mass is the measure of the amount of material in an object. It is measured in grammes, denoted by the symbol g. Everyday units of mass are grammes, kilogrammes, and tonnes (1 tonne = 1000 kg). You will also see the smaller unit of milligrammes used in medicines and other pharmaceuticals.
The masses of atoms and molecules are often expressed in terms of a notional standard atomic mass unit, usually written in biochemistry and molecular biology as a dalton (symbol Da). A dalton is one twelfth of the mass of an atom of the carbon-12 isotope (12C), and is a relative unit rather than being an absolute mass. Large molecules such as proteins typically have masses expressed in kilodaltons (kDa = 1000 Da).

Another relative unit is used in biological- and environmental- chemistry. The 'mole' is the amount of the element or compound that contains a specified number of atoms. The number is called Avagadro's number, and is very large indeed! The resultant unit, written as mol, is useful because it indicates the amount of an element or compound that can combine with another element or compound. The formation of 1 mol of hydrogen chloride (about 36.5 g) results from the combination of 1 mol of chlorine (about 35.5 g) with 1 mol of hydrogen (about 1 g).

We commonly think of mass and weight as interchangeable terms for the same thing. However, weight is a force, that is a product of mass and the gravitational attraction between objects. An object with a mass of 1 g will always have a mass of 1 g. On the surface of the Earth, it will have exert a 'downwards' force that we describe as a 'weight of 1 gramme', whereas on the surface of the Moon that force would be equivalent to a 'weight of 0.16 gramme' on Earth. More properly, the weight should be expressed in units of force, where force is mass times acceleration, denoted as Newtons (symbol N).

The quantity usually called 'density' (occasionally 'specific gravity') is the mass of an object divided by the volume that it occupies. The units for density are mass per unit volume, for example kg m-3 (see the section on Compound units). In everyday speech, we sometimes erroneously describe materials as 'heavy' when we intend to say that they have high density.

Energy and temperature

This part of the web document deals with energy and temperature.

Energy

Energy is found in Nature in many different forms, A basic definition of energy is 'the capacity to do work', and the different forms of energy can often be converted from one to another. The SI unit of energy is the Joule (symbol J). Like the Newton and Hertz, this unit is named after a famous scientist and its symbol is capitalized. In everyday life, you are more likely to meet another, non-SI unit of energy, the calorie (cal). Food labelling shows the energy content of different foodstuffs, usually in units of kcal (1000 cal - also sometimes written confusingly as Calorie). One calorie is just over 4 Joules, and is equivalent to the heat energy needed to raise the temperature of 1 gramme of water by 1°C (see below). So both the Joule and calorie are quite small units.

In biosciences you will meet not only measurements of the quantity of energy, but also the rate at which energy is used or transferred. The Watt (symbol W) is an energy change or transfer of 1 Joule per second (1 J s-1 - see the section on Compound units). Again, we often meet larger or smaller units in everyday life. For instance, the rating of domestic electrical heaters and ovens is given in kilowatts (1 kW = 1000 W).

Various forms of energy may have their own special units, often relating to the effects of the energy source. These include light energy in relation to photosynthetic growth or other biological response, and the effect of exposure to radioactive decay.

Temperature

Temperature scales define how hot or cold objects are. They are established by giving values to the temperatures of specific physical events, such as the freezing or melting points of pure materials. In everyday life, we now use the Celsius temperature scale (sometimes incorrectly called Centigrade). The 'fixed points' for this scale are the freezing point of pure water (0°C) and the boiling point of pure water (100°C).

You may also meet so-called 'absolute' temperatures. These have importance for measurement of physical processes. The unit on the absolute temperature scale is called a Kelvin (symbol K, not °K). One Kelvin represents the same temperature change as one Celsius degree, but the fixed points are different. Thus the freezing point of water (0°C) has a temperature of 273.15 K, whilst the boiling point of water (100°C) is 373.15 K. A temperature of 0 K is commonly called 'absolute zero', at which a physical system neither emits or absorbs energy.

Temperatures on the Fahrenheit scale are still used sometimes, for instance alongside the Celsius scale in TV weather forecasts, and remain commonplace in everyday life in the US. The corresponding fixed points are: freezing point of water = 32°F and boiling point of water = 212°F. Unlike absolute scale, the Fahrenheit degrees are not the same interval as Celsius degrees (1 Celsius degree = 1.8 Fahrenheit degrees).